The partial pressure of the Helium gas is 0.9 atm.
What is the partial pressure of gas collected over water?The pressure that a gas exerts on its own when it is collected over water, independent of the pressure that the water vapor in the collecting vessel also produces, is known as its partial pressure.
When gas is collected over water, some of the water vapor will dissolve in it and change the overall pressure in the collecting vessel. Water vapor has its own partial pressure, which is affected by the relative humidity and temperature of the air around it. This is why it behaves in this way.
We have that;
Vapor pressure of the gas = 19.8 mmHg or 0.026 atm
Partial pressure of the Helium gas = 0.926 atm - 0.026 atm
= 0.9 atm
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Need help matching pairs of structures to diastereomers, enantiomers, constitutional isomers, not isomers, diff representations of the same?
A pair of molecules which exist in two forms that are mirror images of each other but cannot be superimposed one upon the other are called the enantiomers. They are present in pairs and have similar molecular shape.
The compounds with the same molecular formula but are non-superimposable non-mirror images are called diastereomers. They have distinct physical properties and molecular shape.
The constitutional isomers have the same molecular formula but have different bonding atomic organization and bonding patterns.
So here:
1st structure is constitutional isomers (c), 2nd structures are enantiomers (b) and the 3rd are completely different not isomers (d).
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What mass (grams) of magnesium chloride would be formed by the compete reaction of 72.8 grams of magnesium?
Mg +FeCl2 --> Fe + MgCl2
Answer: 285.63g of MgCl2.
Explanation:
Very easy stiochemistry question. Use the dimensional analysis. For example 1 m x 100 cm / 1m and meters get canceled out and 1 m is 100 cm.
For the question, start with the given things. You know that it was started with 72.8 grams of magnesium. Convert it to molar mass (to use moles for comparison), and then find the mass of mg.
Draw a model of the four types of nuclear decay and explain each. Pick the same element (Si-32) to start with.
Sure, I can explain the four types of nuclear decay and provide a model for each using Si-32 as an example.
Si-32 is a radioactive isotope of Silicon with 14 protons and 18 neutrons.
1. Alpha Decay:
In alpha decay, an unstable nucleus emits an alpha particle, which consists of two protons and two neutrons, reducing the atomic number by two and the mass number by four. This makes the resulting nucleus a different element.
Model: Si-32 → alpha particle + Mg-28
Explanation: Si-32 decays into an alpha particle (two protons and two neutrons) and becomes Mg-28.
2. Beta Decay:
In beta decay, a neutron is converted into a proton and an electron. The proton stays in the nucleus, and the electron is emitted as a beta particle. This increases the atomic number by one while keeping the mass number the same.
Model: Si-32 → beta particle + P-32
Explanation: Si-32 decays into a beta particle (an electron) and becomes P-32.
3. Gamma Decay:
Gamma decay occurs when an unstable nucleus emits high-energy photons called gamma rays. Unlike alpha and beta decay, gamma decay does not change the atomic number or mass number of the nucleus.
Model: Si-32 → Si-32 + gamma ray
Explanation: Si-32 emits a gamma ray but remains Si-32.
4. Electron Capture:
In electron capture, an unstable nucleus absorbs an electron from an inner shell, converting a proton into a neutron. This reduces the atomic number by one while keeping the mass number the same.
Model: Si-32 + electron → Al-32
Explanation: Si-32 captures an electron and becomes Al-32.
These four types of nuclear decay can occur in radioactive isotopes, and they result in a change in the atomic number and/or mass number of the nucleus.
what element has 68 degrees Celsius
2. Using the law of conservation of mass, explain why the following reaction is
wrong: HCI + NaOH → NaCl.
According to the law of conservation of mass, the mass of the reactant must be equal to the mass of the product, hence the reaction is wrong
What is the conservation of mass?The law of conservation of mass states that mass within a closed system remains the same over time.
It states that the mass in an isolated system can neither be created nor be destroyed but can be transformed from one form to another.
Thus, the mass of the reactants must be equal to the mass of the products for a low energy thermodynamic process.
From the information given, we have the reaction written as;
HCI + NaOH → NaCl
The mass of the reactant Hydrogen(H) is not found on the product
The mass of the reactant(Oxygen) is also not found
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If the initial temperature of an ideal gas at 2.250 atm
is 62.00 ∘C,
what final temperature would cause the pressure to be reduced to 1.700 atm?
What mass of CO2 can be produced from 25.0 g CaCO3 given the decomposition reaction CaCO3 => CaO + CO2
25.0 g of CaCO3 will produce 11.0 g of CO2. Mass is an intrinsic property of an object, meaning it does not depend on the object's location or the presence of other objects.
What is Mass?
Mass is a measure of the amount of matter in an object. It is a scalar quantity and is typically measured in units such as grams (g) or kilograms (kg). Mass is not the same as weight, which is a measure of the force exerted on an object due to gravity.
The balanced chemical equation for the decomposition of calcium carbonate (CaCO3) is:
CaCO3 → CaO + CO2
According to the equation, 1 mole of CaCO3 produces 1 mole of CO2. The molar mass of CaCO3 is 100.09 g/mol, which means that 1 mole of CaCO3 has a mass of 100.09 g.
To calculate the mass of CO2 produced from 25.0 g of CaCO3, we first need to convert the mass of CaCO3 to moles:
25.0 g CaCO3 x (1 mol CaCO3/100.09 g CaCO3) = 0.2498 mol CaCO3
Since 1 mole of CaCO3 produces 1 mole of CO2, we know that 0.2498 mol of CaCO3 will produce 0.2498 mol of CO2.
To convert the moles of CO2 to mass, we can use the molar mass of CO2, which is 44.01 g/mol:
0.2498 mol CO2 x 44.01 g/mol = 11.0 g CO2
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ASAP!! BRAINLIEST! Please help and show work
Quantifying chemical reactions
Quantifying chemical reactions is essential in understanding the stoichiometry of a reaction, predicting product formation, and optimizing product yield in industrial applications. Stoichiometric coefficients and limiting reactants are two important tools used in this process.
Quantifying chemical reactions involves measuring the amount of reactants and products involved in a chemical reaction. This is important in determining the stoichiometry of the reaction, which refers to the relative amounts of reactants and products involved. Stoichiometry is a crucial concept in chemistry because it allows scientists to predict the amount of product that will be formed from a given amount of reactant, or vice versa.
One way to quantify chemical reactions is through the use of stoichiometric coefficients. These coefficients represent the number of moles of each reactant and product involved in the reaction. For example, the balanced chemical equation for the reaction between hydrogen gas and oxygen gas to form water is:
[tex]2H2 + O2 → 2H2O[/tex]
This equation tells us that two moles of hydrogen gas react with one mole of oxygen gas to form two moles of water. The stoichiometric coefficients can be used to determine the mass of each reactant and product involved in the reaction, using the molar masses of each substance.
Another way to quantify chemical reactions is through the use of limiting reactants. A limiting reactant is the reactant that is completely consumed in a reaction, limiting the amount of product that can be formed. The amount of product formed will be determined by the amount of limiting reactant present. This concept is important in industrial chemistry, where maximizing product yield is often the goal.
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How many grams of O are in 615g of N2O?
There are approximately 223.2 grams of oxygen in 615 grams of N2O.
To find the number of grams of O in 615g of N2O, we first need to understand the chemical formula of N2O. N2O is a compound made up of two nitrogen atoms (N) and one oxygen atom (O). Therefore, the molecular weight of N2O would be:
(2 x atomic weight of N) + (1 x atomic weight of O)
= (2 x 14.01 g/mol) + (1 x 16.00 g/mol)
= 44.01 g/mol
Now, to calculate the number of grams of O in 615g of N2O, we need to know the proportion of O in the compound. Since there is only one oxygen atom in each molecule of N2O, we can find the proportion of O by dividing the atomic weight of O by the molecular weight of N2O:
Atomic weight of O / Molecular weight of N2O
= 16.00 g/mol / 44.01 g/mol
= 0.363
This means that oxygen makes up 36.3% of the total weight of N2O. To find the number of grams of O in 615g of N2O, we can multiply the total weight by the proportion of O:
615g x 0.363
= 223.2g
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Thanks so much to anyone who can help!!!!!!!!!!!
Answer:
1.8mol
Explanation:
this is the ans but in the option there is
not give
How do I find solution concentration
To find the solution concentration, you need to know the amount of solute and the volume of the solution.
The solution concentration is typically expressed in terms of molarity (moles of solute per liter of solution). To calculate the molarity of a solution, divide the moles of solute by the volume of the solution in liters.
Another way to express solution concentration is in terms of percent by mass or volume, which is calculated by dividing the mass or volume of the solute by the mass or volume of the solution and multiplying by 100.
To find the solution concentration, you'll need to calculate the ratio of solute (substance being dissolved) to solvent (substance doing the dissolving) in the mixture.
Concentration is commonly expressed in units like molarity (M), mass/volume percent, or parts per million (ppm).
To calculate molarity (M), divide the moles of solute by the volume of the solvent (in liters). The formula is:
Molarity (M) = moles of solute / volume of solvent (L)
For mass/volume percent, divide the mass of the solute by the total volume of the solution and multiply by 100. The formula is:
Mass/volume percent = (mass of solute / total volume of solution) x 100
For parts per million (ppm), divide the mass of the solute by the total mass of the solution and multiply by 1,000,000.
The formula is:
ppm = (mass of solute / total mass of solution) x 1,000,000
Choose the appropriate formula based on the units required for your specific problem.
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How many grams of magnesium oxide would be formed if 28.2 grams of magnesium was burned?
Mg + O2 --> MgO
When 28.2 grams of Mg is burned, 46.7 grams of MgO will be formed.
How to determine the amount of MgO formed when 28.2 grams of Mg is burnedThe balanced chemical equation for the combustion of magnesium is:
2 Mg + O2 --> 2 MgO
This equation shows that 2 moles of Mg react with 1 mole of O2 to produce 2 moles of MgO.
To determine the amount of MgO formed when 28.2 grams of Mg is burned, we first need to convert the given mass of Mg to moles:
molar mass of Mg = 24.31 g/mol
moles of Mg = mass of Mg / molar mass of Mg
moles of Mg = 28.2 g / 24.31 g/mol
moles of Mg = 1.16 mol
According to the balanced chemical equation, 2 moles of Mg produce 2 moles of MgO. Therefore, we can use the mole ratio to calculate the moles of MgO formed:
moles of MgO = moles of Mg x (2 moles of MgO / 2 moles of Mg)
moles of MgO = 1.16 mol x 1
moles of MgO = 1.16 mol
Finally, we can convert the moles of MgO to grams using its molar mass:
molar mass of MgO = 40.31 g/mol
mass of MgO = moles of MgO x molar mass of MgO
mass of MgO = 1.16 mol x 40.31 g/mol
mass of MgO = 46.7 g
Therefore, when 28.2 grams of Mg is burned, 46.7 grams of MgO will be formed.
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Based on the solubility rules, which one of these phosphate compounds is insoluble in water?
A) Li2CO3
B) Na3PO4
C) Ba(OH)2
D) (NH4)3PO4
(NH4)3PO4 is insoluble in water. The correct option is D
What is solubility rules ?According to their chemical formula and ionic charges, ionic compounds generally follow a set of solubility laws that define their solubility patterns in water. These guidelines aid in determining whether an ionic compound will dissolve in water or not as well as if it will precipitate when combined with other ionic compounds.
Therefore, (NH4)3PO4 is the compound that is expected to be insoluble in water based on the solubility rules.
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In a few sentences, briefly summarize how you were able to determine the amount of Vitamin C in fruit juice using DCPIP.
Haw many valance electrons in the following atoms.
O Na Sr
Answer:O has 6, Na has 1, and Sr has 2.
Explanation:
A helium-filled balloon of the type used in long-distance flying contains 1.5 ✕ 107 L of helium. Let us say you fill the balloon with helium on the ground where the pressure is 837 mm Hg and the temperature is 18.4°C. When the balloon ascends to a height of 6 miles where the pressure is only 707. mm Hg and the temperature is -31°C, what volume is occupied by the helium gas? Assume the pressure inside the balloon matches the external pressure.
We can use the combined gas law to solve this problem:
(P1V1/T1) = (P2V2/T2)
where P1, V1, and T1 are the initial pressure, volume, and temperature, respectively, and P2, V2, and T2 are the final pressure, volume, and temperature, respectively.
We are given that the initial pressure is P1 = 837 mm Hg and the initial volume is V1 = 1.5 × 10^7 L. The initial temperature is T1 = 18.4°C, which we need to convert to Kelvin by adding 273.15:
T1 = 18.4°C + 273.15 = 291.55 K
We are also given that the final pressure is P2 = 707 mm Hg and the final temperature is T2 = -31°C, which we need to convert to Kelvin:
T2 = -31°C + 273.15 = 242.15 K
Now we can solve for the final volume, V2:
(P1V1/T1) = (P2V2/T2)
V2 = (P1V1T2) / (P2T1)
V2 = (837 mm Hg * 1.5 × 10^7 L * 242.15 K) / (707 mm Hg * 291.55 K)
V2 = 5.26 × 10^6 L
Therefore, the volume occupied by the helium gas at the higher altitude is 5.26 × 10^6 L.
How much heat, in joules, would be required to raise the temperature of 450 g of
Aluminum (c Al = 0.21 cal/g o C) from 19.5 o C to 31.2 o C?
Answer:
[tex]\huge\boxed{\sf Q = 1105.65\ cal}[/tex]
Explanation:
Given data:Mass = m = 450 g
T₁ = 19.5 °C
T₂ = 31.2 °C
Change in Temperature = ΔT = 31.2 - 19.5 = 11.7 °C
c = 0.21 cal/g °C
Required:Heat = Q = ?
Formula:Q = mcΔT
Solution:Put the given data in the above formula.
Q = (450)(0.21)(11.7)
Q = 1105.65 cal
[tex]\rule[225]{225}{2}[/tex]
barium reacts with cobalt (iii) cyanide to produce
Answer: Ba + Co(CN)₃ → Ba(CN)₂ + Co₂O₃
Explanation:
Barium reacts with cobalt (III) cyanide to produce barium cyanide and cobalt (III) oxide according to the following chemical equation:
Ba + Co(CN)₃ → Ba(CN)₂ + Co₂O₃
It is a type of displacement reaction.
The iodine monobromide molecule, IBr, has a bond length of 249 pm and a dipole moment of 1.21 D. (a) Which atom of the molecule is expected to have a negative charge? (b) Calculate the effective charges on the I and Br atoms in IBr in units of the electronic charge, e.
a. Br will have the negative charge
b. The effective charges on the I and Br atoms are approximately +1.012e and -1.012e, respectively.
How to determine the negative chargea. To identify which atom within an IBr molecule will have a partial negative charge, we must consider each atom's electronegativity.
On the periodic table, iodine (I) has an electronegativity value of 2.66 while bromine (Br) boasts 2.96; since Br has higher electronegativity it will attract electrons more strongly and hence have an even stronger partial negative charge.
B. To calculate the effective charges on the I and Br atoms in IBr, we can use the dipole moment equation:
μ = Q * d
where μ is the dipole moment, Q is the effective charge, and d is the bond length.
We are given the dipole moment (μ) as 1.21 D, and the bond length (d) as 249 pm. However, we need to convert the units to the SI system before proceeding with the calculation.
[tex]1 D (Debye) = 3.336 * 10^-^3^0 cm,\\\\1 pm = 10^-^1^2 m.[/tex]
Now we can solve for the effective charge (Q):[tex]u = 1.21 D * (3.336 × 10^-^3^0 Cm/D)\\ \\= 4.03656 * 10^-^3^0 cm\\d = 249 pm * (10^-12 m/pm) = 2.49 * 10^-^1^0 m[/tex]
Q = μ / d
[tex]Q = (4.03656 * 10^-^3^0 cm) / (2.49 *10^-^1^0 m) \\\\\\=1.62151 * 10^-^2^0 C[/tex]
This effective charge represents the charge difference between the I and Br atoms. To express the charges in units of the elementary charge (e), we need to divide the effective charge by the elementary charge value (e = 1.602 × 10^-19 C):
Q_e =[tex]\frac{(1.62151 * 10^-^2^0 C)}{(1.602 * 10^-^1^9 C)} = 1.012[/tex]
The effective charges on the I and Br atoms are approximately +1.012e and -1.012e, respectively.
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Solutions of Pb(NO3)2 and NaCl are combined, resulting in concentration of 0.0050 M Pb(NO3)2 and 0.0025 M NaCl immediately upon mixing. Select the correct description of the final solution, given that the Ksp of PbCl2 is 1.70×10^-5.
A. All solutes remain soluble
B. NaNO3 precipitates
C. Pb(NO3)2 precipitates
D. PbCl2 precipitates
Solutions of [tex]Pb(NO_3)^2[/tex] and [tex]NaCl[/tex] are combined, resulting in concentration of 0.0050 M [tex]Pb(NO_3)^2[/tex] and 0.0025 M [tex]NaCl[/tex] immediately upon mixing. The correct description of the final solution, given that the Ksp of [tex]PbCl_2[/tex] is 1.70×10^-5 is All solutes remain soluble. The correct answer is option A
Upon mixing [tex]Pb(NO_3)^2[/tex] and [tex]NaCl[/tex] , the following reaction occurs:
[tex]Pb(NO_3)^2[/tex] + [tex]2NaCl[/tex] → [tex]PbCl_2[/tex] +[tex]2NaNO_3[/tex]
Using the given concentrations of the reactants, the reaction quotient Qc can be calculated as:
Qc =[tex][Pb^2^+][Cl^-]^2[/tex] = [tex](0.0050 M)(0.0025 M)^2[/tex]
Qc [tex]= 3.13[/tex] × [tex]10^{-3}[/tex]
Comparing Qc to the solubility product constant (Ksp) of [tex]PbCl_2[/tex] , we see that Qc < Ksp. This indicates that the system is not at equilibrium and more [tex]PbCl_2[/tex] can dissolve before the product reaches saturation.
Therefore, no precipitation of [tex]PbCl_2[/tex] will occur, and option A is the correct answer: all solutes remain soluble.
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please help show i need help
The complete table for the phase changes would be as follows:
solid to liquid: melting, heating, IMF's breaking, energy absorbedliquid to gas: vaporization, heating, IMF's breaking, energy absorbedsolid to gas: sublimation, heating, IMF's breaking, energy absorbedliquid to solid: freezing, cooling, IMF's forming, energy releasedgas to solid: deposition, cooling, IMF's forming, energy releasedgas to liquid: condensation, cooling, IMF's forming, energy releasedWhat are phase changes?Phase changes occur when a substance changes from one phase to another. When a significant amount of energy is gained or lost, this process takes place.
Phase change also depends on elements like pressure and temperature.
There are six ways a substance can change between these three phases; melting, freezing, evaporating, condensing, sublimation, and deposition.
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Can someone explain the Glyceraldehyde structure for me in detail please. I read that the first carbon atom is the only asymmetric one out of all three carbons and that the other two carbons do have four attachments that just aren’t different. I can’t even see how the atoms have four attachments though.
Answer:
Glyceraldehyde is a simple sugar with three carbon atoms attached to hydroxyl and hydrogen or carbonyl groups. The first carbon atom has four different groups, including an aldehyde group, which makes it asymmetric. This results in two stereoisomers, D-glyceraldehyde and L-glyceraldehyde, that are mirror images of each other and have opposite optical activities.
Difference between practical work inside a laboratory and outside a laboratory?
The main difference between practical work inside and outside a laboratory is the environment and tools used for experimentation.
Practical work inside and outside the laboratoryInside a laboratory, experiments are conducted in a controlled environment with specialized equipment and instruments designed to facilitate experimentation, record data, and ensure safety.
On the other hand, outside the laboratory, experiments are often conducted in a less controlled environment, which can make it more challenging to control variables and obtain accurate results.
Also, experiments outside the laboratory often require different tools and techniques to account for environmental factors such as weather conditions. However, outside the laboratory, there is often more opportunity for real-world applications of experimental findings.
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in an experiment, 1 mol A, 2 mol B and 1 mol D were mixed and allowed to come to equilibrium at 25C. The resulting mixture was found to contain 0.9 mol of C at a total pressure of 1.00 bar. Find the mole fractions of each species at equilibrium
The mole fractions of each species at equilibrium are 0.25 for A and D, 0.5 for B, and 0.225 for C.
we can use the principles of chemical equilibrium and the mole fraction formula.
First, we need to write the balanced chemical equation for the reaction involving A, B, C, and D. Let's assume that the reaction is:
A + 2B <=> C + D
where A, B, C, and D are the chemical species, and the coefficients indicate their stoichiometric ratios.
Next, we need to write the expression for the equilibrium constant, Kc, for this reaction:
Kc = [C][D] / [A][B]²
where [X] denotes the molar concentration of species X at equilibrium.
Since we know the initial moles of A, B, and D, we can calculate their total moles in the mixture:
Total moles = 1 mol A + 2 mol B + 1 mol D = 4 mol
We also know that the final mixture contains 0.9 mol of C. Therefore, the molar concentration of C at equilibrium is:
[C] = 0.9 mol / 4 L = 0.225 M
Since we have only one unknown, we can use the equilibrium constant expression to calculate the molar concentration of D:
Kc = [C][D] / [A][B]²
0.9 = (0.225)(D) / (1)(2²)
D = 1.8
Therefore, the molar concentration of D at equilibrium is 1.8 M.
Using the law of conservation of mass, we can also calculate the molar concentration of A and B at equilibrium:
[A] = 1 mol / 4 L = 0.25 M
[B] = 2 mol / 4 L = 0.5 M
Mole fraction of X = moles of X / total moles
Mole fraction of A = 1 mol / 4 mol = 0.25
Mole fraction of B = 2 mol / 4 mol = 0.5
Mole fraction of C = 0.9 mol / 4 mol = 0.225
Mole fraction of D = 1 mol / 4 mol = 0.25
Therefore, the mole fractions of each species at equilibrium are 0.25 for A and D, 0.5 for B, and 0.225 for C.
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Efficient synthesis in 7 steps or less.
1) Bromination of propylene to form 2-bromopropane using NBS and a Lewis acid catalyst.
What is Bromination?Bromination is a chemical process in which bromine is added to a molecule. This can be done by either direct substitution or as a substitution reaction, allowing for the addition of one or more bromine atoms to the molecule. Bromination is a commonly used organic reaction, particularly in the laboratory, and can be used to alter the properties of a compound. It can also be used to produce a wide range of products, including aromatics and halogenated compounds. Bromination is particularly useful in pharmaceutical synthesis, as the products of this reaction often have desirable bioactivity.
2) Reduction of 2-bromopropane to 2-propanol using NaBH₄
3) Reaction of 2-propanol with phosphorus tribromide to form 2-bromopropanol
4) Alkylation of 2-bromopropanol with methyl iodide to form 2-bromopropyl methyl ether
5) Reduction of 2-bromopropyl methyl ether to 2-methoxypropane using NaBH₄
6) Reaction of 2-methoxypropane with phosphorus tribromide to form 2-bromo-2-methoxypropane
7) Reduction of 2-bromo-2-methoxypropane to Compound X using NaBH₄
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Which best explains why individual chlorine atoms form covalent bonds with each other?
A. to increase their mass
B. to become more reactive
C. to maintain positive charges in their nuclei
D. to have eight electrons in their valence shells
The correct answer is D. to have eight electrons in their valence shells.
What is a covalent bond?A covalent bond is a chemical relationship that requires the sharing of electrons between atoms to generate electron pairs. These electron couples are known as bonding pairs or sharing pairs.
Covalent bonding is the steady balance of attractive and repulsive forces between atoms when they share electrons.
Covalent Bond Types
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Question 28
(1 mark)
Two other minerals can be seen in the photo:
galena, a dark grey mineral with the formula PbS
iron pyrite, a gold-coloured mineral with the formula FeS2
Compare their chemical formulas, by writing down one similarity and one difference between these two minerals.
Note: Pb = lead, Fe = iron, S = sulfur.
Question 29
(1 mark)
Wanting to create the beautiful golden colour of iron pyrite, FeS2, in the lab, a student mixes together black powdered iron (Fe) and yellow powdered sulfur (S). The result is a dull, yellowish grey powder. Propose why this attempt failed?
Question 30
(1 mark)
The student can vary the proportions of iron and sulfur by adding more of each powder to the mixture. Clarify why the same thing isn't true for the compound iron pyrite.
PbS, sometimes referred to as galena, is made up of lead (Pb) and sulfur (S) atoms and has a straightforward structure. Each lead atom forms a tetrahedral link with four sulfur atoms, while each sulfur atom forms a covalent bond with two lead atoms.
Each sulfur atom forms an octahedral link with six iron atoms, while each iron atom forms a covalent bond with two sulfur atoms. FeS2's crystal structure is a cubic, tightly packed lattice.
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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--
N
01H
H
The property of water shown allows it to-
A freeze faster than it boils due to sharing metallic bonds
B. support floating objects due to forces between covalent bonds
C remain stable due to electrons forming ionic bonds
D. be both cohesive and adhesive due to hydrogen bonds
Answer:
D
Explanation:
The special property of water is that it is able to be cohesive and adhesive due to their hydrogen bonds
You have 20.7 grams of water at -25.34 °C. You want to warm it to 155.0 °C. Use the information below to calculate how much heat this will require.
Csolid = 2.09 J/(g·°C)
ΔHfus = 333 J/g
Cvapor = 2.03 J/(g·°C)
ΔHvap = 2260 J/g
Answer:
Cvapor = 2.03 J/(g·°C)heu