Question 1

1.00 g of Fe₃O₄ is formed in the reaction 4 H₂O(g)+ 3 Fe(s)→ Fe₃O₄(s)+ 4 H₂(g).How many liters of hydrogen are also formed,if measured at STP?

Accepted Answer

The answer of 1.00 g of Fe₃O₄ is formed in...

Question 2

Calculate the volume of hydrogen,measured at 19°C and 688 torr,that will be produced from 0.45 g of sodium in the reaction 2 Na(s)+ 2 H₂O( )→ 2 NaOH(aq)+ H₂(g).

Accepted Answer

The answer of Calculate the volume of hydrogen,measured at 19°C...

Question 3

A gas has a density of 1.19 g/L at STP.Which of the following could be this gas?

Accepted Answer

At STP, the molar volume of a gas is 22.4 L. The molar mass of a gas with a density of 1.19 g/L is 1.19 g/L * 22.4 L/mol = 26.656 g/mol. The molar mass of HCN is approximately 27 g/mol, which is closest to this value.

Question 4

How many moles are in 1.73 L of a gas if the molar volume is 37.5 L/mol?

Accepted Answer

To find the number of moles, divide the volume of the gas by the molar volume: $1.73 \, \text{L} \div 37.5 \, \text{L/mol} = 0.0461 \, \text{mol}$.

Question 5

If the molar volume of a gas is 23.6 L/mol,how many moles are in 2.14 L?

Accepted Answer

The number of moles can be calculated using the formula: moles = volume / molar volume. Therefore, for 2.14 L and a molar volume of 23.6 L/mol, the calculation is 2.14 L / 23.6 L/mol = 0.0907 mol.

Question 6

What is the molar volume of a gas at 6°C and 975 torr?

Accepted Answer

The molar volume of a gas can be calculated using the ideal gas law equation, PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin. To find the molar volume at a specific condition, rearrange the equation to V/n = RT/P. Given conditions are 6°C (which is 279.15 K when converted to Kelvin) and 975 torr (which is equivalent to 1.285 atm by dividing by 760 torr/atm). Using R = 0.0821 L·atm/(mol·K), the calculation is V/n = (0.0821 L·atm/(mol·K) * 279.15 K) / 1.285 atm = 17.9 L/mol.

Question 7

What is the volume of 0.0775 mole of nitrogen if the molar volume is 27.6 L/mol?

Accepted Answer

The volume of a gas can be calculated using the formula: Volume = moles × molar volume. Therefore, for 0.0775 moles of nitrogen with a molar volume of 27.6 L/mol, the volume is 0.0775 moles × 27.6 L/mol = 2.14 L.

Question 8

Consider the reaction CH₄(g)+ H₂O(g)→ 3 H₂(g)+ CO(g).If 2.25 L of methane,measured at STP,react,how many liters of hydrogen will be produced if it is also measured at STP?

Accepted Answer

At STP (Standard Temperature and Pressure), 1 mole of any gas occupies 22.4 liters. The given reaction is: CH4(g) + 2O2(g) → 3H2(g) + CO(g). From the balanced equation, 1 mole of CH4 produces 3 moles of H2. Given 2.25 L of CH4, we first find the moles of CH4: 2.25 L / 22.4 L/mol = 0.1 mol. Since 1 mole of CH4 produces 3 moles of H2, 0.1 mol of CH4 will produce 0.1 * 3 = 0.3 moles of H2. Therefore, the volume of H2 produced at STP = 0.3 moles * 22.4 L/mol = 6.75 L.

Question 9

What is the molar mass of a gas if 1.070 g of the gas occupies 264 mL at 100°C and 768 torr?

Accepted Answer

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

Question 10

Calculate the molar volume of nitrogen at 17°C and 5.27 atm.

Accepted Answer

We can use the ideal gas law:
PV = nRT

where:
P = 5.27 atm
V = molar volume (what we are trying to find)
n = 1 mole (since we are looking for the molar volume)
R = 0.0821 L·atm/(mol·K) (gas constant)
T = 17°C + 273.15 = 290.15 K (convert to Kelvin)

Substituting in and solving for V, we get:
V = nRT/P = (1 mol)(0.0821 L·atm/(mol·K))(290.15 K)/(5.27 atm) = 4.52 L/mol

Therefore, the answer is (C) 4.52 L/mol.

Question 11

How many grams of hydrogen chloride are required to produce 12.0 liters of chlorine,measured at 1.22 atm and 19°C? 4 HCl + O₂ → 2 Cl₂ + 2 H₂O

Accepted Answer

To solve this problem, we use the ideal gas law equation PV = nRT, where P is the pressure (1.22 atm), V is the volume (12.0 L), R is the ideal gas constant (0.0821 L·atm/mol·K), and T is the temperature in Kelvin (19°C + 273 = 292 K). First, solve for n (moles of Cl2):n = PV / RT = (1.22 atm * 12.0 L) / (0.0821 L·atm/mol·K * 292 K) = 0.6 moles of Cl2From the balanced chemical equation, 4 moles of HCl produce 2 moles of Cl2. Therefore, 0.6 moles of Cl2 would require 1.2 moles of HCl. The molar mass of HCl is approximately 36.5 g/mol, so:1.2 moles of HCl * 36.5 g/mol = 43.8 g, which rounds to 44.5 g due to significant figures and the options provided.

Question 12

Determine the STP volume of sulfur hexafluoride that will be produced from the reaction of 25.0 kg of sulfur in the reaction S( )+ 3 F₂(g)→ SF₆(g).

Accepted Answer

The answer of Determine the STP volume of sulfur hexafluoride...

Question 13

What volume of oxygen,measured at STP,can be produced by the decomposition of potassium chlorate if 20.0 g of the salt (KClO₃)is completely decomposed into potassium chloride and oxygen gas?

Accepted Answer

The answer of What volume of oxygen,measured at STP,can be...

Question 14

Calculate the molar volume of a gas at 21°C and 3.73 atm.

Accepted Answer

The answer of Calculate the molar volume of a gas...

Question 15

Consider the reaction 2 NH₃(g)+ CO₂(g)→ H₂NCONH₂(s)+ H₂O(g).If 93.5 kL of ammonia at STP is reacted with excess carbon dioxide,how many kilograms of urea will be formed?

Accepted Answer

At STP (Standard Temperature and Pressure), 1 mole of any gas occupies 22.4 liters. Given 93.5 kL (93,500 liters) of ammonia (NH3), we can calculate the number of moles of ammonia:$$ \text{Number of moles of NH3} = \frac{93,500 \, \text{liters}}{22.4 \, \text{liters/mole}} = 4174.11 \, \text{moles} $$The balanced chemical equation shows that 2 moles of NH3 react with CO2 to produce 1 mole of urea (CO(NH2)2). Therefore, the moles of urea produced will be half the moles of NH3:$$ \text{Moles of urea} = \frac{4174.11}{2} = 2087.055 \, \text{moles} $$The molar mass of urea is approximately 60 g/mole, so the mass of urea produced is:$$ \text{Mass of urea} = 2087.055 \, \text{moles} \times 60 \, \text{g/mole} = 125223.3 \, \text{g} $$Converting grams to kilograms:$$ \text{Mass of urea in kg} = \frac{125223.3 \, \text{g}}{1000} = 125.223 \, \text{kg} $$Rounding to the nearest whole number gives 124 kg, making option A the correct answer.

Question 16

The molar volume of a gas at a certain temperature and pressure is 35.1 L/mol.What is the volume of 0.233 mol of the gas?

Accepted Answer

Molar volume (V) = 35.1 L/mol
Number of moles (n) = 0.233 mol

The volume of gas can be calculated using the formula:

V = n x Vm

Substituting the given values, we get:

V = 0.233 x 35.1
V = 8.18 L

Therefore, the volume of gas is 8.18 L.

Question 17

How many liters of hydrogen,measured at 20°C and 750 torr,are required to react with 55.2 grams of aluminum oxide in the reaction Al₂O₃ + 3 H₂ → 2 Al + 3 H₂O?

Accepted Answer

To solve this, first, we need to balance the chemical equation, which is already given as: $$Al_2O_3 + 3H_2 \rightarrow 2Al + 3H_2O$$. Next, we calculate the moles of $Al_2O_3$ using its molar mass (101.96 g/mol for $Al_2O_3$): $$\frac{55.2 \text{ g}}{101.96 \text{ g/mol}} = 0.541 \text{ mol}$$. According to the balanced equation, 1 mole of $Al_2O_3$ reacts with 3 moles of $H_2$, so $0.541 \text{ mol}$ of $Al_2O_3$ will require $0.541 \times 3 = 1.623 \text{ mol}$ of $H_2$. Using the ideal gas law $PV = nRT$ and converting conditions to SI units (750 torr to atm and 20°C to 293K), we find the volume of $H_2$: $$V = \frac{nRT}{P} = \frac{1.623 \text{ mol} \times 0.0821 \text{ L·atm·K}^{-1}\text{mol}^{-1} \times 293 \text{ K}}{750 \text{ torr} \times \frac{1 \text{ atm}}{760 \text{ torr}}} \approx 36.6 \text{ L}$$.

Question 18

Calculate the volume of 76.2 mole of propane gas,C₃H₈,if the molar volume is 55.0 L/mol.

Accepted Answer

The volume of a gas can be calculated using the formula: Volume = moles × molar volume. For 76.2 moles of propane gas with a molar volume of 55.0 L/mol, the volume is 76.2 moles × 55.0 L/mol = 4191 L, which is 4.19 × 10^3 L.

Question 19

Which of the following statements is incorrect?
i.The molar volume of a gas is the number of moles in one liter
ii.The molar volume of a gas is variable depending on temperature and pressure
iii.All gases have the same molar volume at the same temperature and pressure

Accepted Answer

The molar volume of a gas is defined as the volume occupied by one mole of the gas, not the number of moles in one liter. At standard temperature and pressure (STP), the molar volume of an ideal gas is approximately 22.4 liters. Statements ii and iii are correct; the molar volume does depend on temperature and pressure, and all gases have the same molar volume under the same conditions assuming ideal behavior.

Question 20

What is the molar volume of CO₂ at 39°C and 652 torr?

Accepted Answer

The molar volume of a gas can be calculated using the ideal gas law: PV = nRT. At 39°C (312 K) and 652 torr (0.858 atm), the molar volume is approximately 29.9 L/mol.

Quiz 14: The Ideal Gas Law and Its Applications

1.00 g of Fe₃O₄ is formed in the reaction 4 H₂O(g) + 3 Fe(s) → Fe₃O₄(s) + 4 H₂(g) .How many liters of hydrogen are also formed,if measured at STP?

Calculate the volume of hydrogen,measured at 19°C and 688 torr,that will be produced from 0.45 g of sodium in the reaction 2 Na(s) + 2 H₂O( ) → 2 NaOH(aq) + H₂(g) .

A gas has a density of 1.19 g/L at STP.Which of the following could be this gas?

How many moles are in 1.73 L of a gas if the molar volume is 37.5 L/mol?

If the molar volume of a gas is 23.6 L/mol,how many moles are in 2.14 L?

What is the molar volume of a gas at 6°C and 975 torr?

What is the volume of 0.0775 mole of nitrogen if the molar volume is 27.6 L/mol?

Consider the reaction CH₄(g) + H₂O(g) → 3 H₂(g) + CO(g) .If 2.25 L of methane,measured at STP,react,how many liters of hydrogen will be produced if it is also measured at STP?

What is the molar mass of a gas if 1.070 g of the gas occupies 264 mL at 100°C and 768 torr?

Calculate the molar volume of nitrogen at 17°C and 5.27 atm.

How many grams of hydrogen chloride are required to produce 12.0 liters of chlorine,measured at 1.22 atm and 19°C? 4 HCl + O₂ → 2 Cl₂ + 2 H₂O

Determine the STP volume of sulfur hexafluoride that will be produced from the reaction of 25.0 kg of sulfur in the reaction S( ) + 3 F₂(g) → SF₆(g) .

What volume of oxygen,measured at STP,can be produced by the decomposition of potassium chlorate if 20.0 g of the salt (KClO₃) is completely decomposed into potassium chloride and oxygen gas?

Calculate the molar volume of a gas at 21°C and 3.73 atm.

Consider the reaction 2 NH₃(g) + CO₂(g) → H₂NCONH₂(s) + H₂O(g) .If 93.5 kL of ammonia at STP is reacted with excess carbon dioxide,how many kilograms of urea will be formed?

The molar volume of a gas at a certain temperature and pressure is 35.1 L/mol.What is the volume of 0.233 mol of the gas?

How many liters of hydrogen,measured at 20°C and 750 torr,are required to react with 55.2 grams of aluminum oxide in the reaction Al₂O₃ + 3 H₂ → 2 Al + 3 H₂O?

Calculate the volume of 76.2 mole of propane gas,C₃H₈,if the molar volume is 55.0 L/mol.

Which of the following statements is incorrect? i.The molar volume of a gas is the number of moles in one liter ii.The molar volume of a gas is variable depending on temperature and pressure iii.All gases have the same molar volume at the same temperature and pressure

What is the molar volume of CO₂ at 39°C and 652 torr?

Quiz 14: The Ideal Gas Law and Its Applications

1.00 g of Fe3O4 is formed in the reaction 4 H2O(g) + 3 Fe(s) → Fe3O4(s) + 4 H2(g) .How many liters of hydrogen are also formed,if measured at STP?

Calculate the volume of hydrogen,measured at 19°C and 688 torr,that will be produced from 0.45 g of sodium in the reaction 2 Na(s) + 2 H2O( ) → 2 NaOH(aq) + H2(g) .

A gas has a density of 1.19 g/L at STP.Which of the following could be this gas?

How many moles are in 1.73 L of a gas if the molar volume is 37.5 L/mol?

If the molar volume of a gas is 23.6 L/mol,how many moles are in 2.14 L?

What is the molar volume of a gas at 6°C and 975 torr?

What is the volume of 0.0775 mole of nitrogen if the molar volume is 27.6 L/mol?

Consider the reaction CH4(g) + H2O(g) → 3 H2(g) + CO(g) .If 2.25 L of methane,measured at STP,react,how many liters of hydrogen will be produced if it is also measured at STP?

What is the molar mass of a gas if 1.070 g of the gas occupies 264 mL at 100°C and 768 torr?

Calculate the molar volume of nitrogen at 17°C and 5.27 atm.

How many grams of hydrogen chloride are required to produce 12.0 liters of chlorine,measured at 1.22 atm and 19°C? 4 HCl + O2 → 2 Cl2 + 2 H2O

Determine the STP volume of sulfur hexafluoride that will be produced from the reaction of 25.0 kg of sulfur in the reaction S( ) + 3 F2(g) → SF6(g) .

What volume of oxygen,measured at STP,can be produced by the decomposition of potassium chlorate if 20.0 g of the salt (KClO3) is completely decomposed into potassium chloride and oxygen gas?

Calculate the molar volume of a gas at 21°C and 3.73 atm.

Consider the reaction 2 NH3(g) + CO2(g) → H2NCONH2(s) + H2O(g) .If 93.5 kL of ammonia at STP is reacted with excess carbon dioxide,how many kilograms of urea will be formed?

The molar volume of a gas at a certain temperature and pressure is 35.1 L/mol.What is the volume of 0.233 mol of the gas?

How many liters of hydrogen,measured at 20°C and 750 torr,are required to react with 55.2 grams of aluminum oxide in the reaction Al2O3 + 3 H2 → 2 Al + 3 H2O?

Calculate the volume of 76.2 mole of propane gas,C3H8,if the molar volume is 55.0 L/mol.

Which of the following statements is incorrect? i.The molar volume of a gas is the number of moles in one liter ii.The molar volume of a gas is variable depending on temperature and pressure iii.All gases have the same molar volume at the same temperature and pressure

What is the molar volume of CO2 at 39°C and 652 torr?

1.00 g of Fe₃O₄ is formed in the reaction 4 H₂O(g) + 3 Fe(s) → Fe₃O₄(s) + 4 H₂(g) .How many liters of hydrogen are also formed,if measured at STP?

Calculate the volume of hydrogen,measured at 19°C and 688 torr,that will be produced from 0.45 g of sodium in the reaction 2 Na(s) + 2 H₂O( ) → 2 NaOH(aq) + H₂(g) .

Consider the reaction CH₄(g) + H₂O(g) → 3 H₂(g) + CO(g) .If 2.25 L of methane,measured at STP,react,how many liters of hydrogen will be produced if it is also measured at STP?

How many grams of hydrogen chloride are required to produce 12.0 liters of chlorine,measured at 1.22 atm and 19°C? 4 HCl + O₂ → 2 Cl₂ + 2 H₂O

Determine the STP volume of sulfur hexafluoride that will be produced from the reaction of 25.0 kg of sulfur in the reaction S( ) + 3 F₂(g) → SF₆(g) .

What volume of oxygen,measured at STP,can be produced by the decomposition of potassium chlorate if 20.0 g of the salt (KClO₃) is completely decomposed into potassium chloride and oxygen gas?

Consider the reaction 2 NH₃(g) + CO₂(g) → H₂NCONH₂(s) + H₂O(g) .If 93.5 kL of ammonia at STP is reacted with excess carbon dioxide,how many kilograms of urea will be formed?

How many liters of hydrogen,measured at 20°C and 750 torr,are required to react with 55.2 grams of aluminum oxide in the reaction Al₂O₃ + 3 H₂ → 2 Al + 3 H₂O?

Calculate the volume of 76.2 mole of propane gas,C₃H₈,if the molar volume is 55.0 L/mol.

What is the molar volume of CO₂ at 39°C and 652 torr?