The partial pressure of each gas are:
Partial pressure of CH₄ is 1.22 atmPartial pressure of C₂H₆ is 1.46 atmPartial pressure of C₃H₈ is 1.02 atmHow do i determine the partial pressure of each gas?First, we shall determine the mole of 8.00 g of methane, CH₄ and 18.0 g of ethane, C₂H₆. Details below:
For methane, CH₄
Mass of CH₄ = 8 g Molar mass of CH₄ = 16 g/mol Mole of CH₄ =?Mole = mass / molar mass
Mole of CH₄ = 8 / 16
Mole of CH₄ = 0.5 mole
For ethane, C₂H₆
Mass of C₂H₆ = 18 g Molar mass of C₂H₆ = 30 g/mol Mole of C₂H₆ =?Mole = mass / molar mass
Mole of C₂H₆ = 18 / 30
Mole of C₂H₆ = 0.6 mole
Next, we shall determine the total mole. Details below:
Volume (V) = 750 mL = 10 LTemperature (T) = 23 °C = 23 + 273 = 296 KPressure (P) = 3.70Gas constant (R) = 0.0821 atm.L/mol KTotal of mole (n) =?PV = nRT
3.70 × 10 = n × 0.0821 × 293
Divide both sides by (0.0821 × 293)
n = (3.70 × 10) / (0.0821 × 293)
n = 1.52 mole
Finally, we shall determine the partial pressure of each gas. Details below:
For methane, CH₄
Mole of CH₄ = 0.5 moleTotal mole = 1.52 moleTotal pressure = 3.70 atmPartial pressure of CH₄ =?Partial pressure = (Mole / total mole) × total pressure
Partial pressure of CH₄ = (0.5 / 1.52) × 3.70
Partial pressure of CH₄ = 1.22 atm
For ethane, C₂H₆
Mole of C₂H₆ = 0.6 moleTotal mole = 1.52 moleTotal pressure = 3.70 atmPartial pressure of C₂H₆ =?Partial pressure = (Mole / total mole) × total pressure
Partial pressure of C₂H₆ = (0.6 / 1.52) × 3.70
Partial pressure of C₂H₆ = 1.46 atm
For propane, C₃H₈
Partial pressure of CH₄ = 1.22 atmPartial pressure of C₂H₆ = 1.46 atmTotal pressure = 3.70 atmPartial pressure of C₃H₈ =?Partial pressure of C₃H₈ = Total pressure - (Partial pressure of CH₄ + Partial pressure of C₂H₆)
Partial pressure of C₃H₈ = 3.7 - (1.22 + 1.46)
Partial pressure of C₃H₈ = 1.02 atm
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Classify each into the concepts of HEAT and TEMPERATURE
Answer:
Heat HeatHeatTemperatureTemperatureHeat1. What is the percent of NaCl in a mixture that contains 23.5 g of NaCl and 212 g of water? Enter
answers in 2 decimal places
Answer:
9.98%
Explanation:
To find the percent of NaCl in the mixture, we need to divide the mass of NaCl by the total mass of the mixture, and then multiply by 100 to express it as a percentage.
Step 1: Find the total mass of the mixture
total mass = mass of NaCl + mass of water
total mass = 23.5 g + 212 g
total mass = 235.5 g
Step 2: Calculate the percent of NaCl
% NaCl = (mass of NaCl / total mass) x 100
% NaCl = (23.5 g / 235.5 g) x 100
% NaCl = 0.0997876857 x 100
% NaCl = 9.978768677%
% NaCl = 9.98%
Therefore, the percent of NaCl in the mixture is 9.98%.
A 10 g piece of metal at 50°C absorbs 900 G of energy after which the temperature of the metal is 350°C what is the specific heat of the metal
A 10 g piece of metal at 50°C absorbs 900 G of energy after which the temperature of the metal is 350°C. 0.35J/g°C is the specific heat of the metal.
The amount of heat needed to raise a substance's temperature by one degree Celsius in one gramme, also known as specific heat. Typically, calories and joules per gramme per degree Celsius are used as the measurement units of specific heat.
For instance, water has a specific heat of 1 calorie per gramme per degree Celsius. The notion of specific heat was developed by the Scottish scientist Joseph Black in the 18th century as a result of his discovery that equal masses of different substances required varying quantities.
q = m×c×ΔT
900= 10×c×( 350-50)
c=0.35J/g°C
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Compared to chemical reactions, most nuclear reactions result in the
OA. formation of new compounds
OB. formation of new elements
O C. formation of new bonds
OD. loss of valence electrons
Answer:
OB. formation of new elements.
Nuclear reactions involve changes in the nucleus of an atom, such as the splitting of a nucleus or the combining of two nuclei. These reactions can result in the formation of new elements, as the number of protons in the nucleus determines the element. In contrast, chemical reactions involve the rearrangement of electrons between atoms to form new compounds, but do not involve changes to the nucleus.
VITAMIN C IN FRUIT JUICE
Why might it be difficult to use this method to determine the amount of Vitamin C in other fruit juices such as cranberry, blackcurrant, or pomegranate juice?
The method for determining the sum of Vitamin C in fruit juice ordinarily includes adding an indicator (such as DCPIP) to the juice test and titrating the test with a standard arrangement of ascorbic corrosive until the marker changes colour.
In any case, there are a few variables that seem to make this strategy troublesome to utilize for other natural product juices such as cranberry, blackcurrant, or pomegranate juice:
Interference with the indicator: A few natural product juices may contain compounds that are meddled with the marker and anticipate it from changing colour indeed when all the Vitamin C has been titrated. This may lead to wrong comes about.Presence of other reducing agents: Natural product juices may contain other diminishing operators other than Vitamin C, such as fructose or glucose, which can moreover respond with the marker and create wrong positive comes about.Differences in Vitamin C substance: Diverse natural products contain distinctive sums of Vitamin C, and the sum of Vitamin C in a specific juice can change depending on variables such as the readiness of the fruit and the handling strategy utilized. This will make it troublesome to compare the Vitamin C substance of diverse natural product juices utilizing the same strategy.Differences in pH: The pH of natural product juices can moreover change, and this could influence the solidness of Vitamin C and the precision of the titration strategy.In this manner, whereas the strategy for deciding the sum of Vitamin C in natural product juice can be a valuable apparatus, it may not be appropriate for all sorts of natural product juices and may have to be be adjusted or adjusted to account for these variables.
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What is the minimum concentration of fluoride ions necessary to precipitate CaF2 from a 5.25 x 10-3 M solution of Ca(NO3)2? Ksp of CaF2 = 3.9 x 10-11
The minimum concentration of fluoride ions needed is 2.726 x 10⁻⁴ M.
How to solveTo find the minimum concentration of fluoride ions needed to precipitate CaF₂, we'll use the solubility product constant (Ksp) and the calcium ion concentration.
Ksp = [Ca²⁺][F⁻]²
Given: [Ca²⁺] = 5.25 x 10⁻³ M, Ksp = 3.9 x 10⁻¹¹
3.9 x 10⁻¹¹ = (5.25 x 10⁻³)[F⁻]²
Solve for [F⁻]:
[F⁻]² = (3.9 x 10⁻¹¹) / (5.25 x 10⁻³)
[F⁻]² = 7.4286 x 10⁻⁹
[F⁻] = 2.726 x 10⁻⁴ M
The minimum concentration of fluoride ions needed is 2.726 x 10⁻⁴ M.
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Lab: Limiting Reactant and Percent Yield
Step 7: Determine the Limiting Reactant (Trial 2)
Analysis: aluminum
there is no aluminum left
yes
Convert Mass:
2.50g=.019
.25g=.0093
The limiting reactants is/are aluminum.
Are these answers correct?
Yes they are I did the lab.
The given answer statement "there is no aluminum left" and " limiting reactants is aluminum" are correct.
In the analysis of Trial 2, it was found that there was no aluminum left after the reaction had taken place. This indicates that all of the aluminum had reacted with the copper (II) chloride and that it was the limiting reactant in the reaction.
To confirm this, the mass of each reactant was converted to moles using their respective molar masses. It was found that the aluminum had a smaller number of moles than the copper (II) chloride, indicating that it would be used up first and thus be the limiting reactant.
Therefore, the limiting reactant in Trial 2 was aluminum.
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The total pressure of gas collected over water is 725.0 mmHg and the temperature is 18.0 C what is the pressure of hydrogen gas formed in mmHg
The pressure of hydrogen gas formed is 709.5 mmHg.
Partial pressure is the pressure exerted by a single gas component in a mixture of gases, assuming all other gases are held constant.
In this case, the hydrogen gas is formed by a chemical reaction.
To calculate the partial pressure of hydrogen gas, we need to subtract the vapor pressure of water from the total pressure of the gas collected.
The vapor pressure of water at 18.0 °C is 15.5 mmHg.
Therefore, the partial pressure of hydrogen gas can be calculated as:
Partial pressure of hydrogen gas = Total pressure - Vapor pressure of water
Partial pressure of hydrogen gas = 725.0 mmHg - 15.5 mmHg = 709.5 mmHg
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The density of a test gas is to be determined experimentally at 289.2 K using an apparatus constructed of a 4.050 L glass bulb volume that is attached to a vacuum pump. The mass of the evacuated bulb is 22.513 g. After it is filled with the test gas to a pressure of 0.0250 atm, the mass increases to 22.651 g. Assume the gas behaves ideally.
What is the density of the gas? How many moles of gas are in the bulb? What is the apparent molar mass of the gas?
The density of the gas is 0.0340 g/L, moles of gas in the bulb is 0.00124 mol and apparent molar mass is 111.3 g/mol.
How to calculate density, moles and molar mass?To determine the density of the gas, use the ideal gas law:
PV = nRT
where P = pressure, V = volume, n = number of moles, R = gas constant, and T = temperature.
Since the volume and temperature are constant:
(P/n) = constant
Therefore, the density (ρ) of the gas is given by:
ρ = (m-m₀)/V = (Δm)/V
where m = mass of the bulb filled with the gas, m₀ = mass of the evacuated bulb, and Δm = m - m₀ is the mass of the gas.
Substituting the given values:
Δm = 22.651 g - 22.513 g = 0.138 g
V = 4.050 L
ρ = 0.138 g / 4.050 L = 0.0340 g/L
To find the number of moles of gas in the bulb, use the equation:
n = PV/RT
Substituting the given values:
n = (0.0250 atm)(4.050 L) / (0.0821 L·atm/mol·K)(289.2 K) = 0.00124 mol
Finally, to find the apparent molar mass of the gas, use the equation:
M = m/n
where M = molar mass of the gas and m = mass of the gas.
Substituting the given values:
M = 0.138 g / 0.00124 mol = 111.3 g/mol
Therefore, the density of the gas is 0.0340 g/L, there are 0.00124 mol of gas in the bulb, and the apparent molar mass of the gas is 111.3 g/mol.
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Answer the following questions in complete sentences, and justify your responses.
After how many time intervals (shakes) did one-half of your atoms (candies) decay?
What is the half-life of your substance?
If the half-life model decayed perfectly, how many atoms would be remaining (not decayed) after 12 seconds?
If you increased the initial number of atoms (candies) to 300, would the overall shape of the graph be altered? Explain your answer.
Go back to your data table and for each three-second interval, divide the number of candies decayed by the number previously remaining and multiply by 100. Show your work.
The above percentage calculation will help you compare the decay modeled in this experiment to the half-life decay of a radioactive element. Did this activity perfectly model the concept of half-life? If not, was it close?
Compare how well this activity modeled the half-life of a radioactive element. Did the activity model half-life better over the first 12 seconds (four decays) or during the last 12 seconds of the experiment? If you see any difference in the effectiveness of this half-life model over time, what do you think is the reason for it?
To answer these questions, we need to know what substance you are referring to, as well as the data from the experiment.
1. After a certain number of time intervals (shakes), one-half of your atoms (candies) would decay. This number would depend on the specific substance and its half-life.
2. The half-life of a substance is the time it takes for half of its atoms to decay.
3. If the half-life model decayed perfectly, the number of remaining atoms after 12 seconds would depend on the initial number of atoms and the half-life of the substance.
4. If you increased the initial number of atoms (candies) to 300, the overall shape of the graph would not be altered. This is because the half-life decay is a percentage-based process, meaning it would still follow an exponential decay pattern.
5. To calculate the percentage of decay for each three-second interval, you would divide the number of candies decayed by the number previously remaining and multiply by 100. This would show the percentage of decay for each interval.
6. This activity may not perfectly model the concept of half-life, but it can provide a close approximation. Any discrepancies may be due to experimental errors or limitations.
7. To compare how well this activity modeled the half-life of a radioactive element, you would need to analyze the decay percentages over time. If there are differences in the effectiveness of the half-life model, it could be due to the limitations of the experimental setup, such as using candies as a representation of atoms.
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A solution that is neutral has a pH of:
0
14
10
1
7
100 grams of 4 degree celsius water is heated until its temperature is 37 degrees celsius. If the specific heat of water is 4.18 J/g degrees celsius, calculate the amount of heat energy needed to cause this rise in temperature.
To calculate the amount of heat energy needed to cause the rise in temperature, you can use the formula:
Q = mcΔT
Where Q represents the heat energy, m is the mass of the water, c is the specific heat capacity of water, and ΔT is the change in temperature.
Given:
m = 100 grams
c = 4.18 J/g°C
Initial temperature (T1) = 4°C
Final temperature (T2) = 37°C
First, find the change in temperature (ΔT):
ΔT = T2 - T1 = 37°C - 4°C = 33°C
Now, plug the values into the formula:
Q = (100 g) × (4.18 J/g°C) × (33°C)
Q = 13794 J
So, the amount of heat energy needed to cause this rise in temperature is 13,794 Joules.
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2. A slice of chocolate cake contains 560 Calories. a. Determine the number of calories found in the slice of cake. b. Determine the number of joules of energy for the slice of cake. c. Determine the number of kilojoules of energy for the slice of cake. 3. Determine the number of calories in 1.5 kilojoules of energy.
SHIW WORK
b. To determine the number of joules of energy for the slice of cake, we need to convert the calories to joules using the conversion factor 1 calorie = 4.184 joules:
Number of joules = 560 calories * 4.184 joules/calorie = 2343.04 joules
Therefore, the slice of cake contains 2343.04 joules of energy.
c. To determine the number of kilojoules of energy for the slice of cake, we can divide the number of joules by 1000:
Number of kilojoules = 2343.04 joules / 1000 = 2.34304 kilojoules
Therefore, the slice of cake contains 2.34304 kilojoules of energy.
To determine the number of calories in 1.5 kilojoules of energy, we need to convert kilojoules to calories using the conversion factor 1 kilojoule = 1000 calories:
Number of calories = 1.5 kilojoules * 1000 calories/kilojoule = 1500 calories
Therefore, 1.5 kilojoules of energy contains 1500 calories.
Explanation:
Answer:
2. a. 560 Calories, b. 2343.04 J, c. 2.34304 kJ
3. 358.508604 Cal
Explanation:
2.
a. The number of calories found in the slice of chocolate cake is 56012.
b. To determine the number of joules of energy for the slice of cake, we can use the conversion factor that 1 calorie is equal to 4.184 joules3. Therefore, the number of joules in the slice of cake is:
560 Cal ⋅ 4.184 J/ 1 Cal = 2343.04J
c. To determine the number of kilojoules of energy for the slice of cake, we can use the conversion factor that 1 kilojoule is equal to 1000 joules4. Therefore, the number of kilojoules in the slice of cake is:
2343.04 J ⋅ 1 kJ/1000 J = 2.34304 kJ
3. To determine the number of calories in 1.5 kilojoules of energy, we can use the conversion factor that 1 kilojoule is equal to 239.005736 calories1. Therefore, the number of calories in 1.5 kilojoules of energy is:
1.5 kJ ⋅ 239.005736 Cal / 1 kJ = 358.508604 Cal
The hypochlorite ion, ClO-, is the active ingredient in bleach. The perchlorate ion, ClO4-, is a main component of rocket propellants. Draw Lewis structures for both ions.
(a) What is the formal charge of Cl in the hypochlorite ion?
(b) What is the formal charge of Cl in the perchlorate ion, assuming the ClㅡO bonds are all single bonds?
(c) What is the oxidation number of Cl in the hypochlorite ion?
(d) What is the oxidation number of Cl in the perchlorate ion, assuming the ClㅡO bonds are all single bonds?
(e) In a redox reaction, which ion would you expect to be more easily reduced?
(a) The formal charge of Cl in the hypochlorite ion (ClO-) is +1.
(b) The formal charge of Cl in the perchlorate ion (ClO4-) with single bonds is +3.
How to solveFor chlorine (Cl):
Valence electrons: 7
Non-bonding electrons: 6 (3 lone pairs)
Bonding electrons: 2 (1 single bond with oxygen)
Formal charge of Cl = 7 - 6 - (1/2 * 2) = 7 - 6 - 1 = +1
Hence, the formal charge of Cl in the hypochlorite ion is +1.
(c) The oxidation number of Cl in the hypochlorite ion is +1.
(d) The oxidation number of Cl in the perchlorate ion with single bonds is +7.
(e) In a redox reaction, the hypochlorite ion (ClO-) would be more easily reduced because it has a lower oxidation number (+1) compared to the perchlorate ion (+7).
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a solution is made by mixing 100 ml of ethanol and 200 mL of water identified the solute of solvent of the solution and calculate the total volume of the solution
The total volume of the solution is 300 mL.
To calculate the total volume of the solution, we simply add the volumes of the ethanol and water together:
The total volume of solution = volume of ethanol + volume of water
= 100 mL + 200 mL
= 300 mL
Therefore, the total volume of the solution is 300 mL.
When two or more compounds are combined to form a solution, the substance present in the smallest amount is known as the solute, and the material present in the largest amount and which dissolves is known as the solvent.
The solute, which can be a solid, liquid, or gas, dissolves in the solvent, which is often a liquid.
In this scenario, 100 mL of ethanol and 200 mL of water are combined to make the solution. The solute in this solution is ethanol, a colorless liquid. Water is a polar solvent that can dissolve a wide range of compounds, including ethanol. When ethanol and water are combined, they dissolve and form a homogeneous mixture.
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Chemistry Table balance A+B→C
Table 1 attached
The reaction A + B → C has the following rate expression is 197.62 [A][B] M/s
How to determine rate expression?Using the experimental data to determine the order of the reaction with respect to A and B, assume that the rate of the reaction is given by:
rate = [tex]k[A]^x[B]^y[/tex]
where k = rate constant and
x and y = orders of the reaction with respect to A and B, respectively.
Compare the rates of the reaction in trials 1 and 2 while keeping the concentration of A constant:
rate1/rate2 = [tex]\frac{k[A]^x[B]^y}{k[A]^x[B]^y} = \frac{[B]^y}{[B]^y} = 1[/tex]
Conclude that the reaction is first-order with respect to B.
Similarly, compare the rates of the reaction in trials 1 and 3 while keeping the concentration of B constant:
rate1/rate3 =[tex]\frac{k[A]^x[B]^y}{k[A]^x[B]^y} = \frac{[A]^x}{[A]^x} = 1[/tex]
Therefore, the reaction is first-order with respect to A.
The rate expression for the reaction A + B → C is:
rate = k[A][B]
Using any of the experimental trials to determine the value of the rate constant k, use trial 1:
rate1 =[tex]k[A]^1[B]^1[/tex]
k = [tex]\frac{rate1}{[A]^1[B]^1}[/tex] = (3.30 E-3)/(0.012 M x 0.014 M) = 197.62 M⁻² s⁻¹
Therefore, the rate expression for the reaction A + B → C is:
rate = 197.62 [A][B] M/s
In this case, the units of k are M⁻¹ s⁻¹ because the reaction is first-order with respect to both A and B.
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Please help anyone !!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!
The volume of ammonia needed to react completely with 30 Liters of NO at STP is 45 L.
What is the volume of ammonia required in the reaction?
The volume of ammonia needed to react completely with 30 Liters of NO at STP is calculated as follows;
4NH₃ + 6NO → 5N₂ + 6H₂O
From the reaction given above, we can see that;
4 moles of ammonia ------------> 6 moles of NO
ratio = 4 : 6
The volume of ammonia required is calculated as;
4 -------------- > 6
30 L -----------> ?
? = (30 L x 6 ) / 4
? = 45 L
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What is the pH of the solution formed when 12.50 mL of 1.05 M KOH is added to 50.0 mL of 0.225 M HBr?
A. 0.65
B. 1.52
C. 12.48
D. 13.35
Answer: D
Explanation:
When 12.50 mL of 1.05 M KOH is added to 50.0 mL of 0.225 M HBr, the resulting solution has a pH of 13.35.
Here’s how to calculate it:
First, we need to determine the number of moles of KOH and HBr in the solution:
moles of KOH = (12.50 mL) * (1.05 mol/L) * (1 L/1000 mL) = 0.013125 mol moles of HBr = (50.0 mL) * (0.225 mol/L) * (1 L/1000 mL) = 0.01125 mol
KOH is a strong base and HBr is a strong acid, so they will react completely to form water and a salt (KBr):
KOH + HBr -> KBr + H2O
The number of moles of KOH is greater than the number of moles of HBr, so there will be an excess of KOH in the solution after the reaction is complete:
moles of excess KOH = moles of KOH - moles of HBr = 0.013125 mol - 0.01125 mol = 0.001875 mol
The total volume of the solution is the sum of the volumes of KOH and HBr:
total volume = 12.50 mL + 50.0 mL = 62.5 mL
The concentration of excess OH- ions in the solution is:
[OH-] = moles of excess KOH / total volume = 0.001875 mol / (62.5 mL * (1 L/1000 mL)) = 0.03 M
The pOH of the solution can be calculated using the formula pOH = -log[OH-]:
pOH = -log(0.03) = 1.52
The pH can be calculated using the formula pH + pOH = 14:
pH = 14 - pOH = 14 - 1.52 = 13.35
So the correct answer is D. 13.35.
A silver block, initially at 55.1∘C
, is submerged into 100.0 g
of water at 25.0∘C
in an insulated container. The final temperature of the mixture upon reaching thermal equilibrium is 27.9∘C
. The specific heat capacities for water and silver are Cs,water=4.18J/(g⋅∘C)
and Cs,silver=0.235J/(g⋅∘C)
.
The mass of the silver block, given that it was initially at 55.1 °C and is submerged into 100.0 g of water at 25.0°C is 189.8 g
How do i determine the mass of the silver?We'll begin our calculation by obtaining the heat absorbed by the water. Details below:
Mass of water (M) = 100 gInitial temperature (T₁) = 25 °CFinal temperature (T₂) = 27.9 °CChange in temperature (ΔT) = 27.9 - 25 = 2.9 °CSpecific heat capacity of water (C) = 4.184 J/gºC Heat absorbed by water (Q) =?Q = MCΔT
Q = 100 × 4.184 × 2.9
Q = 1213.36 J
Finally, we shall determine the mass of the silver block. Details below:
Heat absorbed by water (Q) = 6108.64 JHeat released by silver block (Q) = -1213.36 JInitial temperature of silver block (T₁) = 55.1 °CFinal temperature of silver block (T₂) = 27.9 °CChange in temperature (ΔT) = 27.9 - 55.1 = -27.2 °C Specific heat capacity of silver (C) = 0.235 J/gºC Mass of silver block (M) =?Q = MCΔT
-1213.36 = M × 0.235 × -27.2
-1213.36 = M × -6.392
Divide both sides by -6.392
M = -1213.36 / -6.392
M = 189.8 g
Thus, we can conclude that the mass of the silver block is 189.8 g
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Complete question:
A silver block, initially at 55.1∘C, is submerged into 100.0 g of water at 25.0∘C in an insulated container. The final temperature of the mixture upon reaching thermal equilibrium is 27.9∘C. The specific heat capacities for water and silver are Cs,water = 4.18J/(g⋅∘C) and Cs, silver = 0.235J/(g⋅∘C). What is the mass of the silver block?
what is the most basic level of organization that can perform functions like converting food into energy
Answer: Cells
Explanation:
Please help thanks!!!!!!!!!!!!!!!!!!
The correct ratio of components is: For every 3 moles of carbon dioxide produced, 5 moles of oxygen react.
This ratio can be derived directly from the balanced chemical equation:
C₃H₈ + 5O₂ → 3CO₂ + 4H₂O
The balanced equation shows that for every 3 moles of carbon dioxide produced, 5 moles of oxygen are required. This means that if we have a certain amount of propane, we need to use this ratio to determine the amount of oxygen needed for the reaction. Similarly, if we have a certain amount of oxygen, we can use this ratio to calculate the amount of carbon dioxide that will be produced.
It is important to note that the other ratios provided in the question are incorrect because they do not match the coefficients in the balanced chemical equation.
Therefore, the correct option is: for every 3 moles of carbon dioxide produced, 5 moles of oxygen react.
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The reactant concentration in a zero-order reaction was 6.00×10−2 M
after 175 s
and 3.50×10−2 M
after 315 s
. What is the rate constant for this reaction?
Chemical equation for the formation of carbonic acid from the reaction of water with carbon dioxide
Answer: H2O + CO2 --> H2CO3
Explanation:
Water and Carbon Dioxide react to form Carbonic Acid
H2O + CO2 --> H2CO3
When calcium metal is placed in water, hydrogen gas is produced. Determine the mass of H2 produced at 25 C and 0.967 atm when 525 mL of the gas is collected over water. Consider vapour pressure of water be 0.0313 atm.
The mass of hydrogen gas produced, given that 525 mL of the gas was collected over water is 0.04 grams
How do i determine the mass of hydrogen gas produced?First, we shall determine the mole of the dry hydrogen gas collected. Details below:
Vapour pressure = 0.0313 atmPressure of wet gas = 0.967 atmPressure of dry gas (P) = 0.967 - 0.0313 = 0.9357 atmTemperature (T) = 25 °C = 25 + 273 = 298 KVolume of gas (V) = 525 mL = 525 / 1000 = 0.525 LGas constant (R) = 0.0821 atm.L/mol KNumber of mole (n) =?PV = nRT
0.9357 × 0.525 = n × 0.0821 × 298
Divide both sides by (0.0821 × 298)
n = (0.9357 × 0.525) / (0.0821 × 298)
n = 0.02 mole
Finally, we shall determine the mass of the hydrogen gas produced. Details below:
Molar mass of hydrogen gas, H₂ = 2 g/mol Mole of hydrogen gas, H₂ = 0.02 moleMass of hydrogen gas, H₂ = ?Mole = mass / molar mass
0.02 = Mass of H₂ / 2
Cross multiply
Mass of H₂ = 0.02 × 2
Mass of hydrogen gas, H₂ = 0.04 grams
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Review-Chemical Reactions
Write balanced chemical equations for the following reactions:
a. chlorine gas and aqueous sodium iodide react to form aqueous sodium chloride and
solid iodine
b. solid sodium chlorate is heated to form solid sodium chloride and oxygen gas
c. solid potassium reacts with liquid water to produce aqueous potassium hydroxide and
hydrogen gas
Answer:
a. Cl2 (g) + 2NaI (aq) → 2NaCl (aq) + I2 (s)
b. 2NaClO3 (s) → 2NaCl (s) + 3O2 (g)
c. 2K (s) + 2H2O (l) → 2KOH (aq) + H2 (g)
Explanation:
Dimensional analysis with shapes
The surface area of the rectangular prism is 0.034 square meters.
For a rectangular prism with length l, width w, and height h, the surface area is:
Surface area = 2lw + 2lh + 2wh
Substituting the given values, we get:
Surface area = 2(10 cm x 5 cm) + 2(10 cm x 8 cm) + 2(5 cm x 8 cm)
Surface area = 100 cm² + 160 cm² + 80 cm² = 340 cm²
We can use dimensional analysis. So the conversion factor is:
1 m² / 10,000 cm²
Multiplying the surface area by this conversion factor, we get:
Surface area = 340 cm² x (1 m² / 10,000 cm²)
Surface area = 0.034 m²
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--The complete Question is, What is the surface area of a rectangular prism that has a length of 10 cm, a width of 5 cm, and a height of 8 cm? Use dimensional analysis to convert the answer to square meters--
5. A sample of unknown metal has a mass of 135 grams. As the sample cools from 100.5 °C to 35.5 °C, it releases 7500 joules of energy. What is the specific heat of the sample?
please show work
The sample of the unknown metal has the mass of the 135 grams. The sample cools from the 100.5 °C to the 35.5 °C, and it releases the 7500 joules of the energy. The specific heat of the sample is 0.854 J/g °C.
Th mass of the metal = 135 g
The initial temperature = 100.5 °C
The final temperature = 35.5 °C
The heat energy releases = - 7500 J
The heat energy is expressed as :
Q = mc ΔT
Where,
The m is mass of the metal = 135 g
The c is the specific heat capacity = ?
The Q is heat energy releases = - 7500 J
The ΔT is the change in the temperature = final temperature - initial temperature.
The ΔT is the change in the temperature = 35.5 - 100.5
The ΔT is the change in the temperature = - 65 °C
The specific heat capacity, c = Q / m ΔT
The specific heat capacity, c = - 7500 / 135 × - 65
The specific heat capacity, c = 0.854 J/g °C
The specific heat capacity of metal is 0.854 J/g °C.
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Which of the following statements confirms the law of conservation of energy?
Statement that shows that the total energy of a system remains constant and is conserved would confirm the law of conservation of energy.
What is law of conservation?
The law of conservation of energy states that energy cannot be created or destroyed, only transformed from one form to another. Therefore, any statement that shows that the total energy of a system remains constant and is conserved would confirm the law of conservation of energy.
Here are some examples of statements that confirm the law of conservation of energy:
The total energy of a closed system, such as a roller coaster, remains constant as the coaster moves from one point to another. Even though the potential energy of the coaster decreases as it goes downhill and the kinetic energy increases, the total energy of the coaster (potential plus kinetic) remains constant.When a pendulum swings back and forth, the potential energy is converted into kinetic energy and back again, but the total energy of the pendulum remains constant.In a chemical reaction, the total energy of the reactants is equal to the total energy of the products. Although energy can be released or absorbed during the reaction, the total energy of the system is conserved.When a ball is thrown into the air, it gains potential energy as it rises and loses potential energy as it falls back down. However, the total energy of the ball (potential plus kinetic) remains constant, neglecting air resistance.All of these statements confirm the law of conservation of energy by showing that the total energy of a system is conserved over time.
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Complete question is: "The total energy of a system remains constant and is conserved" statement would confirm the law of conservation of energy.
Complete combustion of a 0.0200 mol sample of a hydrocarbon, CxHy, gives 4.032 L of CO2 at STP and 3.602 g of H2O.
(a) What is the molecular formula of the hydrocarbon? (b) What is the empirical formula of the hydrocarbon?
The hydrocarbon's molecular structure is [tex]C_9H_20[/tex].The hydrocarbon's empirical formula is [tex]C_9[/tex]/4H5.
To solve this problem, we need to use stoichiometry to relate the amount of [tex]CO__2[/tex] and [tex]H_2O[/tex] produced to the amount of [tex]CxHy[/tex] burned.
(a) To find the molecular formula of the hydrocarbon, we need to first calculate the number of moles of [tex]CO__2[/tex] and [tex]H_2O[/tex] produced. From the ideal gas law, we know that 1 mole of gas at STP (standard temperature and pressure) occupies 22.4 L. Therefore, 4.032 L of [tex]CO__2[/tex] at STP corresponds to:
4.032 L / 22.4 L/mol = 0.180 mol [tex]CO__2[/tex]
Similarly, the mass of H2O produced corresponds to:
3.602 g / 18.02 g/mol = 0.200 mol [tex]H_2O[/tex]
Since the hydrocarbon undergoes complete combustion, it reacts with oxygen to form [tex]CO__2[/tex] and [tex]H_2O[/tex] according to the balanced chemical equation:
[tex]CxHy[/tex] + (x + (y/4))O2 → [tex]CO__2[/tex] + (y/2)[tex]H_2O[/tex]
where x and y are the coefficients of the balanced equation. We can use the stoichiometric ratios to set up two equations:
0.180 mol [tex]CO__2[/tex] = x mol [tex]CxHy[/tex] → x = 0.180 mol / 0.0200 mol = 9
0.200 mol [tex]H_2O[/tex] = (y/2) mol [tex]CxHy[/tex] → y = 0.400 mol / 0.0200 mol = 20
Therefore, the molecular formula of the hydrocarbon is [tex]C_9H_20[/tex].
(b) To find the empirical formula of the hydrocarbon, we need to divide the subscripts by their greatest common factor. In this case, both subscripts are divisible by 4, so we get:
[tex]C_9H_20[/tex] → C9/4H5
Therefore, the empirical formula of the hydrocarbon is C9/4H5.
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d. Given this law, 4 of 4.
Select Choice
of hydrogen (H2) is produced in the following reaction.
Zn + 2HCl → ZnCl2 + H2
65 g 72 g 135 g ?
The mass of hydrogen produced in the reaction is 2g.
What is Mole?The mole is an amount unit similar to familiar units like pair, dozen, gross, etc. It provides a specific measure of the number of atoms or molecules in a bulk sample of matter.
A mole is defined as the amount of substance containing the same number of atoms, molecules, ions, etc. as the number of atoms in a sample of pure 12C weighing exactly 12 g.
Given,
Mass of Zn = 65g
Mass of HCl = 72g
Moles of Zn = mass / molar mass
= 65 / 65 = 1 mole
Moles of HCl = 72 / 36.5
= 1.97 moles
Since moles of Zn is lesser, therefore it is the limiting reagent.
From the reaction, 1 mole of Zn gives 1 mole of hydrogen
Moles of hydrogen = 1 mole
mass of hydrogen = moles × molar mass
= 1 × 2 = 2g
Therefore, the mass of hydrogen produced in the reaction is 2g.
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