9. An unknown gas has a volume of 200L at 5 atm and -140°C. What is its volume at STP?
10. A Los Angeles class nuclear sub has an internal volume of eleven million liter at a
pressure of 1. 250 atm. If a crewman were to open one of the hatches to the outside
ocean while it was underwater (pressure of 15. 75 atm), what would be the new volume
of the air inside?
11. A man heats a balloon in the oven (Why?. Who knows?. It is a crazy world we live in).
If the balloon initially has a volume of 0. 40 L and a temperature of 20 °C, what is its
volume after he heats it to 250 °C?
Mixed Gas Laws
12. A gas has a pressure of 1. 26 atm and occupies a volume of 7. 40 L. If the gas is
compressed to a volume of 2. 93 L, what is its new pressure?
13. People who are angry sometimes say that they feel as if they'll explode. If a calm
person with a lung capacity of 3. 5 liters and a body temperature of 36 °C gets angry,
what is the volume of their lungs if their temperature rises to 39 °C. Do you think they
will really explode?
9. Using the combined gas law, the volume of the gas at STP can be calculated as 112.2 L. This equation takes into account the initial pressure, temperature, and volume, as well as the new pressure and temperature at STP.
10. Applying Boyle's law, the new volume of the air inside the submarine would be approximately 87,873.2 L. This is calculated by multiplying the initial volume and pressure, and dividing by the new pressure.
11. Using the combined gas law, the new volume of the balloon can be calculated as 0.98 L. This equation takes into account the initial temperature, volume, and pressure, as well as the new temperature.
12. Using Boyle's law, the new pressure of the gas can be calculated as 3.25 atm. This equation takes into account the initial pressure and volume, as well as the new volume.
13. Using Charles' law, the new volume of the person's lungs can be calculated as 3.8 L. This equation takes into account the initial lung capacity and temperature, as well as the new temperature.
It is highly unlikely that a person would actually explode from anger, as the body has mechanisms in place to regulate pressure and prevent such an event.
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How many electrons are removed if you ionize one mole of hydrogen using 13. 598V
By considering the concept of Faraday's constant and Avogadro's number we can say that one mole of hydrogen is ionized at 13.598V, removing around 6.022 × 10²³ electrons.
To determine the number of electrons removed when ionizing one mole of hydrogen using 13.598V, we can use the formula:
N = (1 mole) * (Avogadro's number)
where N represents the number of particles (in this case, electrons) in one mole of the substance.
Avogadro's number is approximately 6.022 × 10²³ particles/mol.
Therefore, the number of electrons removed can be calculated as:
N = (1 mole) * (6.022 × 10²³ particles/mol)
= 6.022 × 10²³ electrons
Thus, when ionizing one mole of hydrogen using 13.598V, approximately 6.022 × 10²³ electrons are removed.
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According to the lab introduction in your laboratory manual, the equation for sodium
carbonate dissolving in water is:
3
Na2CO3 + 2H20 – 2Na+ + 2OH- + H2CO3
When this process occurs, sodium carbonate does not 100% separate into ions.
There is always some sodium carbonate in solution.
Based on this reaction, explain whether Sample A or Sample B is most alkaline and
why.
Sample A or Sample B cannot be definitively determined as more alkaline based on the given information. The equation for sodium carbonate dissolving in water shows that it produces both sodium ions (Na⁺) and hydroxide ions (OH⁻), which are the ions responsible for making a solution alkaline.
However, the fact that not all of the sodium carbonate dissociates into ions means that the concentration of alkaline ions in the solution will be less than the total concentration of sodium carbonate added. Therefore, the alkalinity of a sample cannot be determined solely based on the amount of sodium carbonate present.
Other factors, such as the presence of other alkaline substances or the pH of the solution, would need to be considered to determine which sample is more alkaline.
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When water boils, what are the bubbles composed of?.
When water boils, the bubbles are composed of water vapor or steam.
The bubbles form when the water is heated to its boiling point and the water molecules gain enough thermal energy to overcome the intermolecular forces holding them together in the liquid state.
As the water molecules escape into the gaseous state, they form bubbles that rise to the surface of the liquid and release the steam into the atmosphere.
The bubbles are filled with water vapor, which is less dense than liquid water and has a higher thermal energy due to the increased molecular motion in the gas phase. Once the bubbles reach the surface, they burst and release the steam into the air.
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How could you use iron oxide to prepare iron nitrate?
Iron oxide can be reacted with nitric acid to prepare iron nitrate. This reaction involves the displacement of hydrogen ions in nitric acid by iron ions in iron oxide, leading to the formation of iron nitrate and water.
To use iron oxide to prepare iron nitrate, you can follow these steps:
1. Begin with iron oxide (Fe₂O₃), which is a compound consisting of iron and oxygen.
2. Dissolve the iron oxide in a strong acid, such as concentrated nitric acid (HNO₃). This reaction will produce iron nitrate (Fe(NO₃)₃) and water as byproducts. The chemical equation for this reaction is:
2Fe₂O₃ + 6HNO₃ → 4Fe(NO₃)₃ + 3H₂O
3. After the reaction is complete, you can separate the iron nitrate from the remaining mixture by filtration or evaporation. The iron nitrate can then be collected in a crystalline form for further use.
By following these steps, you can successfully use iron oxide to prepare iron nitrate.
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Use the half-reaction method to balance the following equation, which is in an acidic solution: CIO (ag) + I - (ag) -› I (s) + CI- (ag)
The balanced equation using the half-reaction method for the given redox reaction in acidic solution is: CIO₃⁻ (aq) + 3I⁻ (aq) + 6H⁺ (aq) → I₂ (s) + 3CI⁻ (aq) + 3H₂O (l)
The first step in balancing the redox equation using the half-reaction method is to separate the reaction into two half-reactions, one for the oxidation and one for the reduction. In this case, the iodide ion (I⁻) is oxidized to form molecular iodine (I₂) while the chlorate ion (CIO₃⁻) is reduced to form chloride ion (CI⁻). The half-reactions are:
Oxidation half-reaction: I⁻ → I₂
Reduction half-reaction: CIO₃⁻ → CI⁻
Balance the number of atoms of each element in each half-reaction. In the oxidation half-reaction, we have one iodine atom on both sides. In the reduction half-reaction, we have one chlorine atom on both sides. Balance the charges in each half-reaction by adding electrons to the more positive side. In the oxidation half-reaction, we add two electrons to the left side to balance the charge. In the reduction half-reaction, we add six electrons to the left side to balance the charge.
Multiply each half-reaction by a coefficient so that the number of electrons transferred is equal in both half-reactions. In this case, we need to multiply the oxidation half-reaction by three so that it has six electrons, which is the same as the reduction half-reaction. After multiplying and adding the two half-reactions, we get the balanced equation shown above.
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The elephant toothpaste reaction and the reaction of sugar and sulfuric acid are examples of
The elephant toothpaste reaction and the reaction of sugar and sulfuric acid are examples of exothermic reactions and chemical decomposition.
The elephant toothpaste reaction is a popular demonstration in which hydrogen peroxide is mixed with a catalyst, usually potassium iodide or yeast, to rapidly decompose the hydrogen peroxide into oxygen gas and water. This results in the rapid production of a large volume of foam, resembling toothpaste being squeezed from a tube. The reaction is exothermic, meaning it releases heat during the process, causing the foam to be warm or even hot to the touch.
On the other hand, the reaction between sugar (sucrose) and sulfuric acid is an example of a dehydration reaction, which is also exothermic. When concentrated sulfuric acid is added to sugar, it removes the water molecules (H2O) from the sugar, leaving behind a black mass of carbon. The reaction produces a significant amount of heat and steam, making it a visually impressive demonstration.
Both of these reactions showcase the power of chemical decomposition and the release of energy during exothermic reactions. The elephant toothpaste reaction emphasizes the rapid release of gas and foam, while the reaction between sugar and sulfuric acid highlights the process of dehydration and the production of heat.
These reactions provide insight into the various ways that chemical reactions can occur and the diverse range of outcomes that can result from different reactants and conditions.
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What is the rate of change of total pressure in the vessel during the reaction?.
The rate of change of total pressure in a vessel during a reaction depends on the stoichiometry of the reaction and the behavior of the reactants and products with respect to pressure.
In general, if the reaction involves the production or consumption of gases, the total pressure in the vessel will change as the reaction proceeds. The rate of change of total pressure can be calculated using the ideal gas law, which relates the pressure, volume, and temperature of a gas:
PV = nRT
where P is the pressure, V is the volume, n is the number of moles of gas, R is the ideal gas constant, and T is the temperature.
If the number of moles of gas changes during the reaction, the pressure will change accordingly. The rate of change of pressure can be calculated using the following equation:
ΔP/Δt = (Δn/Δt)RT/V
where ΔP/Δt is the rate of change of pressure, Δn/Δt is the rate of change of the number of moles of gas, R is the ideal gas constant, T is the temperature, and V is the volume.
Therefore, to determine the rate of change of total pressure in a vessel during a reaction, it is necessary to know the stoichiometry of the reaction and the behavior of the reactants and products with respect to pressure.
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If 450. 5 calories of heat energy are added to a 89. 6 gram sample of aluminium (specific heat of 0. 215 calories per gram degree celsius) and the initial temperature of the sample is 25. 7 degrees celsius then what is the final temperature in degrees celsius?
The final temperature of an 89.6 gram sample of aluminum is calculated to be 30.6°C after 450.5 calories of heat energy is added, given that the specific heat of aluminum is 0.215 calories per gram degree Celsius and the initial temperature is 25.7°C.
To solve this problem, we can use the formula:
Q = m x c x ΔT
where Q is the amount of heat energy added, m is the mass of the sample, c is the specific heat of the material, and ΔT is the change in temperature.
We are given Q = 450.5 calories, m = 89.6 grams, c = 0.215 calories per gram degree Celsius, and the initial temperature of the sample T1 = 25.7°C.
Let's assume that the final temperature of the sample is T2. Therefore, we can write:
Q = m x c x (T2 - T1)
Solving for T2, we get:
T2 = (Q/mc) + T1
Substituting the given values, we get:
T2 = (450.5 calories)/(89.6 grams x 0.215 calories per gram degree Celsius) + 25.7°C
T2 = 30.6°C
Therefore, the final temperature of the sample is 30.6°C.
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The drinking water in Saplingville was found to contain 13 ppb (parts per billion) of lead. What is the concentration of lead in molarity?
Concentration of lead in Saplingville's drinking water: 6.28 x 10^-11 mol/L.
To calculate the concentration of lead in molarity, we need to follow these steps:
1. Convert ppb (parts per billion) to grams per liter (g/L)
2. Determine the molar mass of lead (Pb)
3. Calculate molarity using the formula: Molarity = (mass in grams / molar mass) / volume in liters
1. Conversion from ppb to g/L:
13 ppb = 13 micrograms/L (µg/L), since 1 ppb = 1 µg/L
13 µg/L = 13 x 10^-9 g/L (since 1 µg = 10^-9 g)
2. Molar mass of lead (Pb) is approximately 207.2 g/mol.
3. Calculate molarity:
Molarity = (13 x 10^-9 g/L) / (207.2 g/mol)
Molarity ≈ 6.28 x 10^-11 mol/L
The concentration of lead in Saplingville's drinking water is approximately 6.28 x 10^-11 mol/L.
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Hydrogen chloride gas (hcl) diffuses 1.8 times faster than an unknown gas. determine the molar mass of the unknown gas.
The molar mass of the unknown gas is approximately 11.25 g/mol.
To determine the molar mass of the unknown gas, we can use Graham's Law of Diffusion.
Graham's law states that the rate of diffusion of a gas is inversely proportional to the square root of its molar mass In other words:
Rate of diffusion of gas A / Rate of diffusion of gas B = sqrt(Molar mass of gas B / Molar mass of gas A)
Using the given information, we can set up an equation:
1.8 (rate of diffusion of unknown gas) / 1 (rate of diffusion of HCl) = sqrt(Molar mass of HCl / Molar mass of unknown gas)
Squaring both sides of the equation, we get:
3.24 = Molar mass of HCl / Molar mass of unknown gas
Multiplying both sides by the molar mass of the unknown gas, we get:
Molar mass of unknown gas = Molar mass of HCl / 3.24
The molar mass of HCl is 36.46 g/mol. Plugging this in, we get:
Molar mass of unknown gas = 36.46 g/mol / 3.24
Molar mass of unknown gas = 11.25 g/mol (rounded to two decimal places)
Therefore, the molar mass of the unknown gas is approximately 11.25 g/mol.
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Which term names the result of two or more atoms combining chemically?.
The term that names the result of two or more atoms combining chemically is a molecule.
A molecule is formed when two or more atoms combine chemically by sharing electrons in a covalent bond.
This bonding occurs when atoms have unpaired electrons in their outermost shell, and they share these electrons to complete their valence shells. In a covalent bond, the electrons are shared between atoms, rather than being transferred, as in an ionic bond.
Molecules can be formed between atoms of the same element or different elements, depending on the chemical properties of the atoms.
For example, two oxygen atoms can combine to form an oxygen molecule (O2), while a hydrogen atom can combine with an oxygen atom to form a water molecule (H2O).
Molecules are the building blocks of all substances in the universe. They are responsible for the chemical and physical properties of substances, such as their melting and boiling points, solubility, and reactivity.
Understanding the formation and behavior of molecules is essential for understanding chemistry and the world around us.
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Part D
Press the yellow reset button at the bottom of the simulation screen. Under Constant Parameter, select Volume. Again,
pump the pump handle once to introduce 40 to 50 gas molecules. Record the pressure in the data table.
Use the heat control to heat the gas to each of the other temperatures in the data table, and record the new pressure.
Answer from Edmentum :)
The instruction is to use the PhET simulation to perform an experiment where the constant parameter is set to volume, and then to pump 40 to 50 gas molecules into the simulation.
The pressure of the gas is recorded in a data table. Next, the heat control is used to heat the gas to each of the other temperatures in the data table, and the corresponding new pressure values are recorded in the data table. This experiment demonstrates the relationship between pressure and temperature, which is known as the ideal gas law.
By holding the volume constant and changing the temperature, we can observe how the pressure of the gas changes. This experiment is useful in understanding real-world phenomena such as how temperature affects the pressure of gas inside a container, such as a tire or a balloon.
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A 983. 6 g sample of antimony undergoes a temperature change of +31. 51 °C. The specific heat capacity of antimony is 0. 049 cal/(g·°C). How many calories of heat were transferred by the sample?
The sample transferred 1,518.7 calories of heat.
First, we need to calculate the heat absorbed or released by the sample using the formula:
q = m * c * ∆T
where q is the heat transferred, m is the mass of the sample, c is the specific heat capacity of antimony, and ∆T is the temperature change.
Plugging in the values, we get:
q = 983.6 g * 0.049 cal/(g·°C) * 31.51 °C
q = 1,518.7 cal
Therefore, the sample transferred 1,518.7 calories of heat.
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A 3. 245g sample of titanium chloride was reacted with sodium metal, producing sodium chloride and metallic titianium. After the sodium chloride was washed out, the remaining titanium metal weighed 0. 819g. What is the empirical formula of the titanium chloride
To find the empirical formula of the titanium chloride, we need to use the given information to determine the moles of titanium and chlorine in the original compound, and then use those values to find the simplest whole-number ratio of atoms in the empirical formula.
First, we can find the moles of titanium in the original compound using the mass of the titanium metal produced:
mass of titanium metal = 0.819 g
molar mass of titanium = 47.867 g/mol
moles of titanium = mass of titanium metal / molar mass of titanium
moles of titanium = 0.819 g / 47.867 g/mol
moles of titanium = 0.0171 mol
Next, we can use the law of conservation of mass to find the moles of chlorine in the original compound:
moles of chlorine = moles of titanium
Now we can find the mass of chlorine in the original compound using the moles of chlorine and the molar mass of chlorine:
moles of chlorine = 0.0171 mol
molar mass of chlorine = 35.453 g/mol
mass of chlorine = moles of chlorine x molar mass of chlorine
mass of chlorine = 0.0171 mol x 35.453 g/mol
mass of chlorine = 0.606 g
Finally, we can use the masses of titanium and chlorine to find the empirical formula of the titanium chloride. The empirical formula gives the simplest whole-number ratio of atoms in a compound, so we need to divide the masses of each element by their respective atomic masses to get the number of moles of each element:
moles of titanium = 0.0171 mol
moles of chlorine = 0.606 g / 35.453 g/mol = 0.0171 mol
The ratio of titanium to chlorine is 1:1, so the empirical formula of the titanium chloride is TiCl<sub>1</sub>, or simply TiCl.
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What is the temperature of a gas at 100 kPa if the gas had a temperature of
26°C at 200 kPa?
The temperature of the gas at 100 kPa is approximately 149.575 K.
The temperature of a gas at 100 kPa, when it initially had a temperature of 26°C at 200 kPa, can be determined using the combined gas law. The combined gas law relates the initial and final pressures, volumes, and temperatures of a gas, and can be written as:
(P1 * V1) / T1 = (P2 * V2) / T2
where P1 and P2 are the initial and final pressures, V1 and V2 are the initial and final volumes, and T1 and T2 are the initial and final temperatures.
In this case, we are given the initial pressure (P1 = 200 kPa), initial temperature (T1 = 26°C), and final pressure (P2 = 100 kPa). We can convert the initial temperature to Kelvin by adding 273.15, so T1 = 26°C + 273.15 = 299.15 K.
Since the problem does not specify any changes in volume, we can assume that the volume remains constant (V1 = V2). This simplifies the equation to:
(P1 * V) / T1 = (P2 * V) / T2
Canceling out the volume terms (V) on both sides:
P1 / T1 = P2 / T2
Now, we can solve for the final temperature, T2:
T2 = (P2 * T1) / P1
T2 = (100 kPa * 299.15 K) / 200 kPa
T2 ≈ 149.575 K
Therefore, the temperature of the gas at 100 kPa is approximately 149.575 K.
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The industrial production of hydroiodic acid takes place by treatment of iodine with hydrazine N2H4: 2I2 + N2H4 = 4HI + N2 a) how many grams of I2 needed to react with 36. 7 g of N2H4? b) how many grams of HI are produced from the reaction of 115. 7 g of N2H4 with excess iodine?
a) To determine the number of grams of I2 needed to react with 36.7 g of N2H4, we need to use stoichiometry.
The balanced equation for the reaction is:
2I2 + N2H4 → 4HI + N2
From the equation, we can see that 2 moles of I2 react with 1 mole of N2H4 to produce 4 moles of HI. So, the mole ratio of I2 to N2H4 is 2:1.
First, we need to determine the number of moles of N2H4 in 36.7 g:
moles of N2H4 = mass / molar mass
moles of N2H4 = 36.7 g / 32.045 g/mol
moles of N2H4 = 1.146 mol
Since the mole ratio of I2 to N2H4 is 2:1, we need half as many moles of I2 as there are moles of N2H4:
moles of I2 = 1.146 mol / 2
moles of I2 = 0.573 mol
Finally, we can calculate the number of grams of I2 needed:
mass of I2 = moles of I2 x molar mass of I2
mass of I2 = 0.573 mol x 253.81 g/mol
mass of I2 = 145.5 g
Therefore, 145.5 grams of I2 are needed to react with 36.7 grams of N2H4.
b) To determine the number of grams of HI produced from the reaction of 115.7 g of N2H4 with excess iodine, we need to use stoichiometry again.
The balanced equation for the reaction is:
2I2 + N2H4 → 4HI + N2
From the equation, we can see that 2 moles of I2 react with 1 mole of N2H4 to produce 4 moles of HI. So, the mole ratio of HI to N2H4 is 4:1.
First, we need to determine the number of moles of N2H4 in 115.7 g:
moles of N2H4 = mass / molar mass
moles of N2H4 = 115.7 g / 32.045 g/mol
moles of N2H4 = 3.609 mol
Since the mole ratio of HI to N2H4 is 4:1, we can calculate the number of moles of HI produced:
moles of HI = 4 x moles of N2H4
moles of HI = 4 x 3.609 mol
moles of HI = 14.436 mol
Finally, we can calculate the number of grams of HI produced:
mass of HI = moles of HI x molar mass of HI
mass of HI = 14.436 mol x 127.91 g/mol
mass of HI = 1846.5 g
Therefore, 1846.5 grams of HI are produced from the reaction of 115.7 grams of N2H4 with excess iodine.
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Elemental silicon is oxidized by o2 to give a compound which dissolves in molten na2co3. when this solution is treated with aqueous hydrochloric acid, a precipitate forms. what is the precipitate
Elemental silicon is oxidized by O₂ to give a compound which dissolves in molten Na₂CO₃. when this solution is treated with aqueous hydrochloric acid, a precipitate forms. silica gel is the precipitate.
The compound formed by the oxidation of elemental silicon with O₂ is silicon dioxide (SiO₂), which can dissolve in molten Na₂CO₃ to form sodium silicate (Na₂SiO₃).
When this solution is treated with aqueous hydrochloric acid (HCl), the sodium silicate reacts with the HCl to form a precipitate of silica gel (SiO₂·nH₂O). This reaction is known as the gelatinization of sodium silicate. The sodium chloride (NaCl) formed by the reaction remains in solution.
The silica gel precipitate is often used as a desiccant or drying agent due to its high surface area and ability to adsorb water molecules.
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`Name:
Date:
Properties of Matter - Crunch time Review
1. If two objects balance like the ones shown below, what must be true?
A. Object A has more mass than object B.
Both objects have the same mass.
C. Object A has more volume than object B.
D. Both objects have the same volume.
Answer:
d
Explanation:
because i did it
How many moles of ice will form if 105 kJ of heat is removed from liquid
water at 0°C? The enthalpy of solidification for water is 6.01 kJ/mol.
17.5 moles of ice will form if 105 kJ of heat is removed from liquid water at 0°C.
What is moles?Moles are small, burrowing mammals that belong to the Talpidae family. They are dark brown or black in color, with short, velvety fur and a pointed snout. Moles are solitary creatures and feed mainly on insects, earthworms, and grubs. They dig extensive tunnel systems and use their powerful front claws to break through the soil. Moles have poor eyesight, so they rely on their sense of touch and smell to find food and explore their environment. They are found in many parts of the world, including North America, Europe, and Asia. Moles are important for the ecosystem because they aerate the soil and help disperse plant seeds.
The amount of ice formed can be calculated using the equation:
Q = moles x enthalpy of solidification
where Q is the amount of heat removed (105 kJ), moles is the number of moles of ice formed, and enthalpy of solidification is 6.01 kJ/mol.
Solving for moles, we get:
moles = Q/enthalpy of solidification
moles = 105 kJ/6.01 kJ/mol
moles = 17.5 moles.
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Complete the balanced chemical equation for the following reaction between a weak acid and a strong base. HClO₂(aq) + Ba (OH)₂(aq) →
The balanced chemical equation for the reaction between a weak acid, HClO₂, and a strong base, Ba(OH)₂, is:
2 HClO₂(aq) + Ba(OH)₂(aq) → Ba(ClO₂)₂(aq) + 2 H₂O(l)
The balanced chemical equation for the reaction between a weak acid, HClO₂, and a strong base, Ba(OH)₂, is:
2 HClO₂(aq) + Ba(OH)₂(aq) → Ba(ClO₂)₂(aq) + 2 H₂O(l)
In this reaction, the Ba(OH)₂ dissociates completely into Ba²⁺ and 2 OH⁻ ions in solution. The HClO₂ is a weak acid and therefore only partially dissociates into H⁺ and ClO₂⁻ ions in solution. The reaction between these ions forms Ba(ClO₂)₂, a salt, and water.
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A 54.2 g sample of Magnesium has an initial temperature of 55°C and a final temperature of 78°C, and the specific heat of Magnesium is 1.023 J/g°C. If the sample absorbs 1300 J of heat energy, what is the change in temperature?
Change in temperature of the Magnesium sample is calculated as 23.7°C.
What is meant by heat energy?Heat energy is a form of energy that is transferred between objects or systems due to temperature difference. It flows from hotter to cooler objects, and its amount is measured in joules.
As we know; Q = m c ΔT
Q is the amount of heat absorbed, m is mass of the object, c is specific heat, and ΔT is change in temperature.
ΔT = Q / (m * c)
ΔT = 1300 J / (54.2 * 1.023 )
ΔT = 23.7°C
Therefore, the change in temperature of the Magnesium sample is 23.7°C.
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A solution consisting of 11. 4 g NH4Cl in 150 ml of water is titrated with 0. 20 M KOH.
a. How many milliliters of KOH are required to reach the equivalence point?
b. Calculate {Cl-], [K+], and [NH3] at the equivalence point. Assume volumes are additive
a.It requires 1066 mL of 0.20 M KOH to reach the equivalence point.
b.The equivalence point, the concentration of [Cl-], [K+], and [[tex]NH_{3}[/tex]] in the solution, is 0.175 M.
What is the Equivalence point?
The chemical equivalent between the added titrant and the sample analyte is called the equivalence point in a titration.
a. We need to know how many moles of [tex]NH_{4}Cl[/tex] are in the solution to calculate the volume of 0.20 M KOH needed to achieve the equivalence point.
First, we can determine how many moles [tex]NH_{4}Cl[/tex] are present in the solution:
moles [tex]NH_{4}Cl[/tex] = mass / molar mass
moles [tex]NH_{4}Cl[/tex] = 11.4 g / 53.49 g/mol (molar mass of [tex]NH_{4}Cl[/tex])
moles [tex]NH_{4}Cl[/tex] = 0.2132 mol
At the equivalence point, all the [tex]NH_{4}Cl[/tex] has interacted with the KOH, resulting in an equal amount of moles of [tex]NH_{3}[/tex] and [tex]H_{2} O[/tex]. This suggests that 0.2132 moles of KOH are also needed to react with [tex]NH_{4}Cl[/tex] The volume of 0.20 M KOH required to react with 0.2132 mol can be determined using the equation for the reaction between [tex]NH_{4}Cl[/tex] and KOH:
[tex]NH_{4}Cl[/tex] + KOH → [tex]NH_{3}[/tex] + [tex]H_{2}O[/tex] + KCl
moles KOH = moles [tex]NH_{4}Cl[/tex]
= 0.2132 mol
volume of KOH = moles KOH / concentration of KOH
= 0.2132 mol / 0.20 mol/L
= 1.066 L or 1066 mL
Therefore, 1066 mL of 0.20 M KOH is required to reach the equivalence point.
b. At the equivalence point, an equal amount of moles of KOH and [tex]NH_{4}Cl[/tex] interacted to create [tex]NH_{3}[/tex], [tex]H_{2}O[/tex], and KCl.
We may determine the concentration of [Cl-] and [K+] in the solution following the reaction at the equivalence point by assuming volumes are additive:
moles KCl = moles [tex]NH_{4}Cl[/tex]
= 0.2132 mol
volume of solution = 150 mL + volume of KOH added
= 150 mL + 1066 mL
= 1216 mL
= 1.216 L
[Cl-] = moles KCl / volume of solution
[Cl-] = 0.2132 mol / 1.216 L
[Cl-] = 0.175 M
[K+] = moles KCl / volume of solution
[K+] = 0.2132 mol / 1.216 L
[K+] = 0.175 M
The fact that the reaction between [tex]NH_{4}Cl[/tex]and KOH is a one-to-one reaction can be used to compute the concentration of [[tex]NH_{3}[/tex]]. As a result, 0.2132 mol of NH3 is likewise created at the equivalence point. Using the overall volume of the solution, we can get the [[tex]NH_{3}[/tex]] concentration:
[[tex]NH_{3}[/tex]] = moles [tex]NH_{3}[/tex]/ total volume of solution
[[tex]NH_{3}[/tex]] = 0.2132 mol / 1.216 L
[[tex]NH_{3}[/tex]] = 0.175 M
Therefore, at the equivalence point, the concentration of [Cl-], [K+], and [[tex]NH_3}[/tex]] in the solution is 0.175 M.
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Help what’s the answer?
The product is HI
There are six product molecule
Hydrogen is the limiting reactant
There is one iodine molecule in excess
How do you know limiting reactant?To determine the limiting reactant in a chemical reaction, you need to compare the number of moles of each reactant present to the stoichiometry of the balanced chemical equation.
The limiting reactant is the reactant that is completely consumed in a chemical reaction, and which therefore limits the amount of product that can be formed. The other reactant, which is not completely consumed, is called the excess reactant.
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A chemist interested in the efficiency of a chemical reaction would calculate the:.
A chemist interested in the efficiency of a chemical reaction would calculate the c. percentage yield.
The percentage yield compares the actual yield of a reaction to the theoretical yield and indicates how efficient the reaction is in producing the desired product. It is calculated by dividing the actual yield by the theoretical yield and multiplying by 100 to express it as a percentage.
The other options listed are also important measurements in chemistry but are not directly related to assessing the efficiency of a reaction:
a. Mole ratio: The mole ratio is a ratio that indicates the stoichiometric relationship between the reactants and products in a chemical reaction. It is used to determine the relative amounts of substances involved in a reaction, but it does not directly measure the efficiency of the reaction.
b. Energy released: This refers to the energy that is released or absorbed during a chemical reaction. While energy considerations are important, they do not directly measure the efficiency of the reaction.
d. Rate of reaction: The rate of reaction refers to how quickly a chemical reaction occurs, which is an important factor but not the direct measurement of efficiency. The rate of reaction can be influenced by factors such as temperature, concentration, and catalysts, but it does not provide information about the overall efficiency of the reaction in terms of yield.
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Complete question :
A chemist interested in the efficiency of a chemical reaction would calculate the :
a. mole ratio.
b. energy released.
c. percentage yield.
d. rate of reaction.
Question 1 options: calculate the energy, in joules, of a photon that has a frequency of 3.73 x 1014 s-1.
The energy of a photon can be calculated using the equation E = hf, where E is the energy of the photon, h is Planck's constant, and f is the frequency of the photon.
Substituting the given values, we get:
E = (6.626 x 10⁻³⁴ J s) x (3.73 x 10¹⁴ s⁻¹)
E = 2.47 x 10⁻¹⁹ J
Therefore, the energy of the photon with a frequency of 3.73 x 10¹⁴ s¹ is 2.47 x 10⁻¹⁹ J.
This value may seem small, but it is consistent with the fact that photons with higher frequencies (and thus higher energies) are required to cause certain types of chemical reactions and ionization processes.
The energy of a photon with a frequency of 3.73 x 1010¹⁴ s¹ is calculated using the equation E = hf, where h is Planck's constant. The energy of the photon is found to be 2.47 x 1010⁻¹⁹ J.
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(01. 05 MC)
During an experiment a thermometer was placed in a beaker containing hydrogen peroxide. The following observations were recorded when yeast granules were added to hydrogen peroxide.
Observation 1: Fizzing and bubbling took place.
Observation 2: The temperature began to rise.
Based on the observation, justify the type of change (physical or chemical) that took place
When yeast granules were added to hydrogen peroxide, two observations were made: fizzing and bubbling took place, and the temperature began to rise. These observations suggest that a chemical change occurred.
Chemical changes involve a transformation of the molecular structure of a substance, resulting in the formation of new substances with different properties. In this case, the hydrogen peroxide likely reacted with the yeast granules to produce oxygen gas and water, which caused the fizzing and bubbling.
The increase in temperature may be a result of the energy released during the chemical reaction.
Physical changes, on the other hand, involve a change in the physical state or appearance of a substance, without any alteration to its molecular structure. For example, melting ice is a physical change, as the solid ice changes to liquid water, but the molecules themselves remain unchanged.
In summary, the observations of fizzing and bubbling, as well as the temperature increase, suggest that a chemical change occurred when yeast granules were added to hydrogen peroxide. This change likely involved the production of oxygen gas and water.
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which of the following options correctly describe the oxidation of primary alcohols? select all that apply. multiple select question. primary alcohols require different oxidizing conditions than secondary alcohols. a carboxylic acid can be produced by oxidation of a primary alcohol. during oxidation, a primary alcohol will rearrange to produce a more substituted oxidation product. mild oxidizing conditions will result in an aldehyde product. harsher oxidizing conditions will produce a ketone from a primary alcohol.
The options that describe the oxidation of the primary alcohols is a carboxylic acid can be produced by oxidation of a primary alcohol. Mild oxidizing conditions will result in an aldehyde product.
The Primary alcohols will be oxidized to form the aldehydes and the carboxylic acids. The secondary alcohols will be oxidized to give the ketones. The Tertiary alcohols, in the contrast, cannot be oxidized by without breaking the molecules of the C–C bonds.
The Primary alcohols and the aldehydes will be normally oxidized to the carboxylic acids using the potassium dichromate solution in the presence of the dilute sulfuric acid that is H₂SO₄.
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What is the empirical formula for a compound that is 94. 1% oxygen and 5. 90 % hydrogen?
The empirical formula for this compound is H1O1.
To find the empirical formula of a compound with 94.1% oxygen and 5.9% hydrogen, we first assume a 100g sample. This gives us 94.1g of oxygen and 5.9g of hydrogen. Next, we'll convert these values to moles:
Oxygen: 94.1g / 16g/mol (molar mass of O) ≈ 5.88 moles
Hydrogen: 5.9g / 1g/mol (molar mass of H) ≈ 5.9 moles
Now, we'll find the mole ratio by dividing both values by the smallest number of moles:
Oxygen: 5.88 / 5.88 ≈ 1
Hydrogen: 5.9 / 5.88 ≈ 1
The empirical formula for this compound is H1O1, which can be simplified to H2O (water).
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Classify the following size particle: 4.2cm
I need an answer no explanation needed
Particle size is typically measured in units such as micrometers (µm) or nanometers (nm), which represent very small lengths on the order of thousandths or millionths of a meter, respectively.
What is the classification of the particle?4.2 cm is much larger than the typical size of particles and is more in the range of everyday objects.
For example, 4.2 cm is roughly the size of a golf ball or a small tomato. If you have additional information about the particle's size, such as its shape or the material it is made of, I may be able to provide more specific guidance.
Also, a particle that is 4.2 nanometers (nm) in size falls in the range of nanoscale particles, which are typically much smaller than everyday objects and are invisible to the nakεd eye.
The size of the particle can provide some clues about its potential identity or classification, but additional information about its properties, composition, and context is needed to determine its specific identity.
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