Question 1

Phosgene (98.92 g/mol)can be formed from carbon monoxide (28.01 g/mol)and chlorine gas (70.90 g/mol)according to the following reaction: CO(g)+ Cl₂(g)$\to$ COCl₂(g) How many grams of COCl₂ can be produced when 0.772 atm CO and 0.753 atm Cl₂ are mixed in a 260 L tank at 323 K,assuming 100% yield?

Accepted Answer

The balanced chemical equation is:CO(g) + Cl2(g) → COCl2(g)The mole fraction of CO is:XCO = PCO / (PCO + PCl2) = 0.772 atm / (0.772 atm + 0.753 atm) = 0.507The mole fraction of Cl2 is:XCl2 = PCl2 / (PCO + PCl2) = 0.753 atm / (0.772 atm + 0.753 atm) = 0.493The total number of moles of gas in the tank is:n = (P * V) / (R * T) = (1.525 atm * 260 L) / (0.0821 L atm / mol K * 323 K) = 12.5 molThe number of moles of COCl2 produced is:nCOCl2 = XCO * n = 0.507 * 12.5 mol = 6.34 molThe mass of COCl2 produced is:mCOCl2 = nCOCl2 * MW = 6.34 mol * 98.92 g/mol = 626 gTherefore, the correct answer is A: 760 g.

Question 2

The density of a gaseous compound of nitrogen and oxygen is 4.11 g/L at STP.What is the most likely formula of this gas?

Accepted Answer

The answer of The density of a gaseous compound of...

Question 3

Hydrogen sulfide gas (H₂S,34.08 g/mol)can be produced from the reaction of aluminum sulfide (150.2 g/mol)and water (18.02 g/mol)according to the following reaction equation: Al₂S₃(s)+ 6 H₂O( )$\to$ 3 H₂S(g)+ 2 Al(OH)₃(s) If 65.0 g Al₂S₃ reacts with excess H₂O at 90.0S1U1P1$\circ$S1S1P0C and 0.987 atm,what volume of H₂S gas will be produced?

Accepted Answer

The answer of Hydrogen sulfide gas (H₂S,34.08 g/mol)can be produced...

Question 4

You wish to monitor the progress of a reaction using pressures.Suppose 17.06 g N₂ (28.02 g/mol)and 1.228 g H₂ (2.016 g/mol)are initially present in a 20.0 L reaction vessel at 127S1U1P1$\circ$S1S1P0C.Nitrogen and hydrogen can react to form ammonia (17.04 g/mol)according to the reaction shown.At a given point,the total pressure (the sum of the pressures of N₂,H₂,and NH₃ present)is 1.48 atm.What percentage of the initial N₂ has reacted? N₂(g)+ 3 H₂(g)$\to$ 2 NH₃(g)

Accepted Answer

To find the percentage of N2 that has reacted, first calculate the initial moles of N2 and H2. Then, use the ideal gas law to find the initial total pressure. With the given total pressure at a certain point, determine the change in moles due to the reaction. Calculate the moles of N2 that have reacted and find the percentage of the initial moles.

Question 5

The density of an unknown gas is 1.72 g/L at 750.0 torr and 30.0S1U1P1$\circ$S1S1P0C.Which of the following could be the unknown gas?

Accepted Answer

The ideal gas law can be used to solve for the molar mass (M) of the unknown gas:
PV = nRT
n = m/M
PM/RT = ρ
M = ρRT/P
Assuming standard temperature and pressure (STP), we can convert the density to the molar mass of the gas. STP is defined as 0°C (273.15K) and 1 atm (760 torr).
ρSTP = (1.72 g/L) (273.15K/303.15K) (1 atm/750.0 torr) = 0.0902 g/L
Using this molar mass, we can compare it to the molar masses of the answer choices:
A) CS2: M = 76.14 g/mol
B) NO: M = 30.01 g/mol
C) NSO: M = 76.06 g/mol
D) NH3: M = 17.03 g/mol
E) NO2: M = 46.01 g/mol
The closest molar mass is that of NSO, so the unknown gas is most likely NSO.

Question 6

One compound under investigation for use as a lightweight rocket fuel is dimethylhydrazine (60.10 g/mol).It reacts with dinitrogen tetroxide (92.01 g/mol)according to the following reaction: (CH₃)₂N₂H₄( )+ N₂O₄( )$\to$ 3 N₂(g)+ 4 H₂O(g)+ 2 CO₂(g) If 150 g (CH₃)₂N₂H₄ react with excess N₂O₄ at 473 K and 760 torr,what volume of CO₂ gas will form?

Accepted Answer

The answer of One compound under investigation for use as...

Question 7

What is the density of sulfur hexafluoride (SF₆,146.1 g/mol)in a cylinder at 1.5 atm and 22S1U1P1$\circ$S1S1P0C?

Accepted Answer

To solve for density, we can use the ideal gas law: PV=nRT, where P is pressure, V is volume, n is the number of moles, R is the gas constant, and T is temperature in Kelvin. We can rearrange the ideal gas law to solve for density: density= (n x M)/V, where M is the molar mass of the gas. Since the volume and number of moles are not given, we can assume that they are constant and cancel out in the equation. Thus, the density is directly proportional to the pressure and inversely proportional to the temperature.

We need to convert the temperature to Kelvin: 22°C + 273.15 = 295.15 K.

density= (n x M)/V = (1 x 146.1 g/mol) / [(1 atm / 1.5 atm) x (295.15 K / 273.15 K)] = 9.1 g/L

Therefore, the answer is B.

Question 8

What is the density of propane gas (CH₃CH₂CH₃,44.1 g/mol)at 25S1U1P1$\circ$S1S1P0C and 650 mmHg?

Accepted Answer

To solve for density, we can use the ideal gas law: PV = nRT. We can rearrange this equation to solve for density: d = (molar mass) * (P/RT). Plugging in the given values, we get:
d = (44.1 g/mol) * (650 mmHg / (0.0821 L*atm/mol*K * (25+273.15) K))
d = 1.54 g/L
Therefore, the answer is A (1.54 g/L).

Question 9

Which of the following reactions will result in a reduced total pressure if run to completion?

Accepted Answer

The answer of Which of the following reactions will result...

Question 10

Suppose 3.95% of 521 g PCl₅ (208.2 g/mol)initially present in a 10.0 L reaction vessel at 300S1U1P1$\circ$S1S1P0C decomposes to form PCl₃ (137.3 g/mol)and Cl₂ (70.90 g/mol).What is the resulting pressure of PCl₃? PCl₅(g)$\to$ PCl₃(g)+ Cl₂(g)

Accepted Answer

To find the pressure of PCl₃, first calculate the moles of PCl₅ decomposed: 3.95% of 521 g is 20.56 g. Convert this to moles: 20.56 g / 208.2 g/mol = 0.0988 mol. Since the decomposition is 1:1, moles of PCl₃ formed = 0.0988 mol. Use PV=nRT to find pressure: P = (nRT)/V. With R = 0.0821 L·atm/mol·K and T = 300 K, P = (0.0988 mol * 0.0821 * 300 K) / 10.0 L = 0.243 atm.

Question 11

Hydrogen gas (2.02 g/mol)can be produced from the reaction of methane (16.05 g/mol)and water vapor (18.02 g/mol)according to the following reaction equation: CH₄(g)+ H₂O(g)$\to$ CO(g)+ 3 H₂(g) If 262 g CH₄ react with excess H₂O at 423 K and 0.862 atm,what volume of H₂ gas will form?

Accepted Answer

Using stoichiometry, 262 g of CH₄ is 16.32 moles. From the balanced equation, 1 mole of CH₄ produces 3 moles of H₂. Therefore, 16.32 moles of CH₄ will produce 48.96 moles of H₂. Using the ideal gas law (PV=nRT), with R=0.0821 L·atm/mol·K, T=423 K, and P=0.862 atm, the volume V = (nRT)/P = (48.96 * 0.0821 * 423) / 0.862 = 1970 L.

Question 12

Which of the following gases has nearly the same density as CO₂ at room temperature and atmospheric pressure?

Accepted Answer

N₂O has a molar mass of 44 g/mol, which is very close to the molar mass of CO₂ (44 g/mol), making their densities nearly the same under similar conditions.

Question 13

Which container shown below has the largest partial pressure of helium? The white circles represent helium atoms; the dark circles represent argon atoms.

Accepted Answer

Container C has the largest partial pressure of helium because it has the highest concentration of helium atoms compared to the other containers. Container A has a similar number of helium atoms as container C, but it also has more argon atoms, which will lower the overall partial pressure of helium. Containers B and D have fewer helium atoms than container C, and container E cannot be determined without additional information.

Question 14

What is the molar mass of a gas that has a density of 3.123 g/L at STP?

Accepted Answer

The answer of What is the molar mass of a...

Question 15

Which one of the following gases could most easily be differentiated from propane (CH₃CH₂CH₃)on the basis of density when compared at the same temperature and pressure?

Accepted Answer

Propane (C3H8) has a molar mass of 44.1 g/mol while fluorine gas (F2) has a molar mass of 38.0 g/mol. Therefore, at the same temperature and pressure, fluorine gas will have a lower density than propane and can be easily differentiated from propane based on density. The other gases listed (CO, NO, and N2O) have molar masses that are relatively close to propane and would not show a significant difference in density at the same temperature and pressure.

Question 16

Calcium carbonate (100.1 g/mol)decomposes according to the following reaction: CaCO₃(s)$\to$ CaO(s)+ CO₂(g) What pressure of CO₂ gas will form in a 25.0 mL jar containing 5.00 g CaCO₃ at 300 K if 0.00500% of the solid decomposes?

Accepted Answer

First, calculate the moles of CaCO3 that decompose: 5.00 g * 0.00500% = 0.00025 g. Convert to moles: 0.00025 g / 100.1 g/mol = 2.50 x 10^-6 mol. Using the ideal gas law (PV = nRT), with R = 0.0821 L·atm/mol·K and V = 0.025 L, the pressure P = (2.50 x 10^-6 mol * 0.0821 * 300 K) / 0.025 L = 2.46 x 10^-3 atm.

Question 17

Nitrous oxide (N₂O,44.02 g/mol)has been used as an anesthetic.What is the density of N₂O at 750 torr and 30.0S1U1P1$\circ$S1S1P0C?

Accepted Answer

The answer of Nitrous oxide (N₂O,44.02 g/mol)has been used as...

Question 18

What is the molar mass of a gas that has a density of 2.62 g/L at 2.00 atm and 25.0S1U1P1$\circ$S1S1P0C?

Accepted Answer

We can use the ideal gas law to solve for the molar mass, where PV = nRT. We can rearrange this to solve for n/V, which is the molarity:

n/V = P/RT

We are given the density, which is mass/volume, so we can rewrite n/V as:

n/V = mass/(volume x molar mass)

Substituting in the given values and solving for molar mass:

2.62 g/L = (2.00 atm x 1.01325 bar/atm x 101.325 Pa/bar) / ((273.15 + 25) K) x (1 mol/1,000 g) / M

M = 32.1 g/mol

Question 19

Butane and oxygen were allowed to completely react at 540 torr and 298 K.After the exothermic reaction,620 L of CO₂ are collected at 823 K and 750 torr.How many liters of O₂ gas at 540 torr and 298 K were consumed? 2 C₄H₁₀(g)+ 13 O₂(g)$\to$ 8 CO₂(g)+ 10 H₂O(g)

Accepted Answer

The answer of Butane and oxygen were allowed to completely...

Question 20

The partial pressure of a gas is __________

Accepted Answer

The partial pressure of a gas is the pressure due to that gas in a mixture. It is not the pressure the gas exerts when pure (A), necessarily the same as the vapor pressure (B), the total pressure of a mixture of gases (D), nor the pressure exerted by one molecule of the gas (E).

Quiz 10: Properties of Gases-The Air We Breathe

The density of a gaseous compound of nitrogen and oxygen is 4.11 g/L at STP.What is the most likely formula of this gas?

The density of an unknown gas is 1.72 g/L at 750.0 torr and 30.0^$\circ$C.Which of the following could be the unknown gas?

What is the density of sulfur hexafluoride (SF₆,146.1 g/mol) in a cylinder at 1.5 atm and 22^$\circ$C?

What is the density of propane gas (CH₃CH₂CH₃,44.1 g/mol) at 25^$\circ$C and 650 mmHg?

Which of the following reactions will result in a reduced total pressure if run to completion?

Suppose 3.95% of 521 g PCl₅ (208.2 g/mol) initially present in a 10.0 L reaction vessel at 300^$\circ$C decomposes to form PCl₃ (137.3 g/mol) and Cl₂ (70.90 g/mol) .What is the resulting pressure of PCl₃? PCl₅(g) $\to$ PCl₃(g) + Cl₂(g)

Which of the following gases has nearly the same density as CO₂ at room temperature and atmospheric pressure?

Which container shown below has the largest partial pressure of helium? The white circles represent helium atoms; the dark circles represent argon atoms.

What is the molar mass of a gas that has a density of 3.123 g/L at STP?

Which one of the following gases could most easily be differentiated from propane (CH₃CH₂CH₃) on the basis of density when compared at the same temperature and pressure?

Calcium carbonate (100.1 g/mol) decomposes according to the following reaction: CaCO₃(s) $\to$ CaO(s) + CO₂(g) What pressure of CO₂ gas will form in a 25.0 mL jar containing 5.00 g CaCO₃ at 300 K if 0.00500% of the solid decomposes?

Nitrous oxide (N₂O,44.02 g/mol) has been used as an anesthetic.What is the density of N₂O at 750 torr and 30.0^$\circ$C?

What is the molar mass of a gas that has a density of 2.62 g/L at 2.00 atm and 25.0^$\circ$C?

Butane and oxygen were allowed to completely react at 540 torr and 298 K.After the exothermic reaction,620 L of CO₂ are collected at 823 K and 750 torr.How many liters of O₂ gas at 540 torr and 298 K were consumed? 2 C₄H₁₀(g) + 13 O₂(g) $\to$ 8 CO₂(g) + 10 H₂O(g)

The partial pressure of a gas is __________

Quiz 10: Properties of Gases-The Air We Breathe

The density of a gaseous compound of nitrogen and oxygen is 4.11 g/L at STP.What is the most likely formula of this gas?

The density of an unknown gas is 1.72 g/L at 750.0 torr and 30.0 ∘\circ∘ C.Which of the following could be the unknown gas?

What is the density of sulfur hexafluoride (SF6,146.1 g/mol) in a cylinder at 1.5 atm and 22 ∘\circ∘ C?

What is the density of propane gas (CH3CH2CH3,44.1 g/mol) at 25 ∘\circ∘ C and 650 mmHg?

Which of the following reactions will result in a reduced total pressure if run to completion?

Suppose 3.95% of 521 g PCl5 (208.2 g/mol) initially present in a 10.0 L reaction vessel at 300 ∘\circ∘ C decomposes to form PCl3 (137.3 g/mol) and Cl2 (70.90 g/mol) .What is the resulting pressure of PCl3? PCl5(g) →\to→ PCl3(g) + Cl2(g)

Hydrogen gas (2.02 g/mol) can be produced from the reaction of methane (16.05 g/mol) and water vapor (18.02 g/mol) according to the following reaction equation: CH4(g) + H2O(g) →\to→ CO(g) + 3 H2(g) If 262 g CH4 react with excess H2O at 423 K and 0.862 atm,what volume of H2 gas will form?

Which of the following gases has nearly the same density as CO2 at room temperature and atmospheric pressure?

Which container shown below has the largest partial pressure of helium? The white circles represent helium atoms; the dark circles represent argon atoms.

What is the molar mass of a gas that has a density of 3.123 g/L at STP?

Which one of the following gases could most easily be differentiated from propane (CH3CH2CH3) on the basis of density when compared at the same temperature and pressure?

Calcium carbonate (100.1 g/mol) decomposes according to the following reaction: CaCO3(s) →\to→ CaO(s) + CO2(g) What pressure of CO2 gas will form in a 25.0 mL jar containing 5.00 g CaCO3 at 300 K if 0.00500% of the solid decomposes?

Nitrous oxide (N2O,44.02 g/mol) has been used as an anesthetic.What is the density of N2O at 750 torr and 30.0 ∘\circ∘ C?

What is the molar mass of a gas that has a density of 2.62 g/L at 2.00 atm and 25.0 ∘\circ∘ C?

Butane and oxygen were allowed to completely react at 540 torr and 298 K.After the exothermic reaction,620 L of CO2 are collected at 823 K and 750 torr.How many liters of O2 gas at 540 torr and 298 K were consumed? 2 C4H10(g) + 13 O2(g) →\to→ 8 CO2(g) + 10 H2O(g)

The partial pressure of a gas is __________

The density of an unknown gas is 1.72 g/L at 750.0 torr and 30.0^$\circ$C.Which of the following could be the unknown gas?

What is the density of sulfur hexafluoride (SF₆,146.1 g/mol) in a cylinder at 1.5 atm and 22^$\circ$C?

What is the density of propane gas (CH₃CH₂CH₃,44.1 g/mol) at 25^$\circ$C and 650 mmHg?

Suppose 3.95% of 521 g PCl₅ (208.2 g/mol) initially present in a 10.0 L reaction vessel at 300^$\circ$C decomposes to form PCl₃ (137.3 g/mol) and Cl₂ (70.90 g/mol) .What is the resulting pressure of PCl₃? PCl₅(g) $\to$ PCl₃(g) + Cl₂(g)

Which of the following gases has nearly the same density as CO₂ at room temperature and atmospheric pressure?

Which one of the following gases could most easily be differentiated from propane (CH₃CH₂CH₃) on the basis of density when compared at the same temperature and pressure?

Calcium carbonate (100.1 g/mol) decomposes according to the following reaction: CaCO₃(s) $\to$ CaO(s) + CO₂(g) What pressure of CO₂ gas will form in a 25.0 mL jar containing 5.00 g CaCO₃ at 300 K if 0.00500% of the solid decomposes?

Nitrous oxide (N₂O,44.02 g/mol) has been used as an anesthetic.What is the density of N₂O at 750 torr and 30.0^$\circ$C?

What is the molar mass of a gas that has a density of 2.62 g/L at 2.00 atm and 25.0^$\circ$C?

Butane and oxygen were allowed to completely react at 540 torr and 298 K.After the exothermic reaction,620 L of CO₂ are collected at 823 K and 750 torr.How many liters of O₂ gas at 540 torr and 298 K were consumed? 2 C₄H₁₀(g) + 13 O₂(g) $\to$ 8 CO₂(g) + 10 H₂O(g)