Question 1

A balloon is filled with He gas to a volume of 2.10 L at 35 °C.The balloon is placed in liquid nitrogen until its temperature reaches -196 °C.Assuming the pressure remains constant,what is the volume of the cooled balloon?

Accepted Answer

According to Charles' law, at constant pressure, the volume of a gas is directly proportional to its temperature in Kelvin. We need to convert both the initial and final temperatures to Kelvin: 35 °C + 273.15 = 308.15 K and -196 °C + 273.15 = 77.15 K.

So, we can set up the proportion:

V1 / T1 = V2 / T2

where V1 = 2.10 L, T1 = 308.15 K, and T2 = 77.15 K. Solving for V2 gives:

V2 = (V1 x T2) / T1 = (2.10 L x 77.15 K) / 308.15 K = 0.525 L

Therefore, the volume of the cooled balloon is 0.525 L.

Question 2

What volume of oxygen will react with 21 mL of ethanol,assuming the gases are present at the same temperature and pressure? 2 CH₃CH₂OH(g)+ 6 O₂(g)→ 4 CO₂(g)+ 6 H₂O(g)

Accepted Answer

The balanced chemical equation given is: $$2 C_2H_5OH(g) + 6 O_2(g) \rightarrow 4 CO_2(g) + 6 H_2O(g)$$. According to the stoichiometry of the reaction, 2 moles of ethanol react with 6 moles of oxygen. Therefore, for 21 mL of ethanol, the volume of oxygen required, assuming gases are at the same temperature and pressure (and thus directly proportional to moles), would be $\frac{21 \text{ mL ethanol} \times 6 \text{ moles oxygen}}{2 \text{ moles ethanol}} = 63 \text{ mL oxygen}$.

Question 3

A 2.00-L glass soda bottle filled only with air is tightly capped at 19°C and 732.0 mmHg.If the bottle is placed in water at 89°C,what is the pressure in the bottle?

Accepted Answer

The pressure in the bottle can be found using the ideal gas law and the concept that the amount of gas and the volume of the container are constant. The relationship between initial and final conditions is given by $P_1/T_1 = P_2/T_2$, where $P$ is pressure, $T$ is temperature in Kelvin, and subscripts 1 and 2 refer to initial and final conditions, respectively. Convert temperatures to Kelvin: $T_1 = 19°C + 273 = 292K$ and $T_2 = 89°C + 273 = 362K$. Solve for $P_2$: $P_2 = P_1 \times (T_2/T_1) = 732.0 \text{ mmHg} \times (362K / 292K) \approx 907 \text{ mmHg}$.

Question 4

A 26.4-L sample of nitrogen at 7.50 atm and 24°C is simultaneously expanded to 58.4 L and heated to 35°C.What is the new pressure of the gas?

Accepted Answer

The answer of A 26.4-L sample of nitrogen at 7.50...

Question 5

Equal volumes of propane,C₃H₈,and carbon monoxide,CO,at the same temperature and pressure have the same ____.

Accepted Answer

According to Avogadro's law, equal volumes of gases at the same temperature and pressure contain the same number of molecules. Therefore, propane (C3H8), carbon disulfide (CS2), and carbon monoxide (CO) will have the same number of molecules under these conditions.

Question 6

The pressure of O₂ in a 15.0 L flask is 322 mm Hg at 44 °C.What mass of O₂ is in the flask? (R = 0.08206 L⋅atm/mol⋅K)

Accepted Answer

First, convert the pressure from mm Hg to atm: 322 mm Hg * (1 atm / 760 mm Hg) = 0.4237 atm. Convert the temperature from Celsius to Kelvin: 44 °C + 273.15 = 317.15 K. Use the ideal gas law: PV = nRT. Solve for n (moles of O2): n = PV / RT = (0.4237 atm * 15.0 L) / (0.08206 L⋅atm/mol⋅K * 317.15 K) = 0.244 mol. The molar mass of O2 is 32.00 g/mol, so the mass is 0.244 mol * 32.00 g/mol = 7.82 g.

Question 7

The temperature of a specific amount of gas in a sealed container changes from 40.0°C to 80.0°C.If the volume remains constant,the pressure will change from 755 mmHg to ___.

Accepted Answer

The pressure of a gas is directly proportional to its temperature in Kelvin when the volume is constant (Gay-Lussac's Law). To find the final pressure, convert the temperatures to Kelvin and use the formula P1/T1 = P2/T2. Initial temperature = 40.0°C = 313.15 K, final temperature = 80.0°C = 353.15 K. Initial pressure = 755 mmHg. Solving for P2 gives P2 = (755 mmHg) * (353.15 K / 313.15 K) ≈ 851 mmHg.

Question 8

What is the pressure of a 52.5-L gas sample containing 1.57 mol of gas at 93.2°C? (R = 0.0821 L • atm/(K • mol),1 atm = 760 mmHg)

Accepted Answer

First, we need to convert the temperature to Kelvin: 
93.2°C + 273.15 = 366.35 K

Then, we can use the ideal gas law to solve for pressure: 
PV = nRT

P = nRT/V

P = (1.57 mol)(0.0821 L•atm/(K•mol))(366.35 K)/(52.5 L)

P = 6.83 × 1012 Pa

Finally, we can convert Pa to mmHg:

1 Pa = 0.0075 mmHg

P = 6.83 × 1012 Pa x 0.0075 mmHg/Pa

P = 5.12 × 1010 mmHg

Rounding to two significant figures, we get an answer of 6.8 x 1010 mmHg, which corresponds to choice D.

Question 9

What is the final volume of nitrogen gas if the pressure of 5.8 L of the gas is decreased to one-half of its original pressure,and its absolute temperature is increased to double the original temperature?

Accepted Answer

According to the combined gas law, (P1 * V1) / T1 = (P2 * V2) / T2. If the pressure is halved (P2 = P1/2) and the temperature is doubled (T2 = 2T1), the final volume V2 = (P1 * V1 * 2T1) / (P1/2 * T1) = 4 * V1 = 4 * 5.8 L = 23.2 L, which rounds to 23 L.

Question 10

What volume is occupied by 35.0 g of C₂H₂ at 471 mm Hg and 21 °C? (R = 0.08206 L⋅atm/mol⋅K)

Accepted Answer

The answer of What volume is occupied by 35.0 g...

Question 11

A gas occupying a volume of 1.50 L exerts a pressure of 700 mmHg at 200°C.Which mathematical expression gives the correct pressure at 9.00 L and 350°C?

Accepted Answer

The answer of A gas occupying a volume of 1.50...

Question 12

A 45.0 L gas cylinder contains 988 g He at 23 °C.What is the pressure inside the cylinder? (R = 0.08206 L⋅atm/mol⋅K)

Accepted Answer

The answer of A 45.0 L gas cylinder contains 988...

Question 13

You have a 30.0 L cylinder of helium at a pressure of 132 atm and a temperature of 19 °C.The He is used to fill balloons to a volume of 1.80 L at 745 mm Hg and 27 °C.How many balloons can be filled with He? Assume that the cylinder can provide He until its internal pressure reaches 1.00 atm (i.e.,there are 131 atmospheres of usable He in the cylinder).

Accepted Answer

The answer of You have a 30.0 L cylinder of...

Question 14

Gaseous chlorine is held in two separate containers at identical temperatures and pressures.The volume of container 1 is 1.30 L,and it contains 6.70 mol of the gas.The volume of container 2 is 2.75 L.How many moles of the gas are in container 2?

Accepted Answer

Using the ideal gas law, the number of moles is directly proportional to the volume at constant temperature and pressure. Therefore, (6.70 mol / 1.30 L) = (x mol / 2.75 L), solving for x gives 14.2 mol.

Question 15

If 0.357 g of CH₄ gas is introduced into an empty 1.75 L flask at 25 °C,what will be the pressure inside the flask? (R = 0.08206 L⋅atm/mol⋅K)

Accepted Answer

First, we need to calculate the number of moles of the gas:

n = m/M = 0.357 g / 78.17 g/mol = 0.00456 mol

Next, we can use the ideal gas law to solve for the pressure:

PV = nRT

P = nRT/V

P = (0.00456 mol)(0.08206 L·atm/mol·K)(298 K)/(1.75 L)

P = 0.311 atm

Therefore, the pressure inside the flask is 0.311 atm. The answer is C).

Question 16

You have 34.5 g of O₂ gas in a container with twice the volume as one with CO₂ gas.The pressure and temperature of both containers are the same.Calculate the mass of carbon dioxide gas you have in the container.

Accepted Answer

Using the ideal gas law and the fact that the number of moles is proportional to the volume for gases at the same temperature and pressure, the mass of CO2 is half that of O2 because the volume is half. Therefore, the mass of CO2 is 34.5 g / 2 = 17.25 g. However, the molar mass of CO2 is 44 g/mol, and for O2 it is 32 g/mol. Adjusting for molar mass, the mass of CO2 is (34.5 g * 44 g/mol) / (32 g/mol) / 2 = 23.7 g.

Question 17

Which of the following gases has the greatest density at 35 °C and 450 mm Hg?

Accepted Answer

The density of a gas is directly related to its molar mass under the same conditions of temperature and pressure. Among the given options, Cl₂ (molecular weight approximately 70.9 g/mol) has the highest molar mass, which means it has the greatest density at the specified conditions.

Question 18

The volume of a sample of gas measured at 50.0°C and 1.00 atm pressure is 2.00 L.What must the final temperature be in order for the gas to have a final volume of 3.00 L at 1.00 atm pressure?

Accepted Answer

To find the final temperature for the gas to have a final volume of 3.00 L at the same pressure, we use Charles's Law, which states that $V_1/T_1 = V_2/T_2$, where $V$ is volume, $T$ is temperature in Kelvin, and the subscripts 1 and 2 refer to the initial and final states, respectively. First, convert the initial temperature to Kelvin: $50.0°C + 273.15 = 323.15 K$. Then, solve for $T_2$: $T_2 = (V_2/V_1) \times T_1 = (3.00 L / 2.00 L) \times 323.15 K = 484.725 K$. Convert back to Celsius: $484.725 K - 273.15 = 211.575°C$, which rounds to 211.5°C.

Question 19

What volume of gaseous silane,SiH₄,has the same moles of gas as 9.00 L of helium gas at the same temperature and pressure?

Accepted Answer

According to Avogadro's law, equal volumes of gases at the same temperature and pressure contain the same number of moles. Therefore, 9.00 L of helium gas will have the same number of moles as 9.00 L of silane gas under the same conditions.

Question 20

What volume does 49.0 g of N₂ gas occupy at STP? (R = 0.08206 L⋅atm/mol⋅K)

Accepted Answer

To use the ideal gas law to solve for volume, we need to know the number of moles of gas present, which can be found by dividing the mass by the molar mass. The molar mass of N₂ can be calculated by adding up the atomic masses of each element in the formula: molar mass = (1 x atomic mass of N) + (1 x atomic mass of S) + (12 x atomic mass of U) + (1 x atomic mass of B) molar mass = (1 x 14.01 g/mol) + (1 x 32.06 g/mol) + (12 x 238.03 g/mol) + (1 x 10.81 g/mol) molar mass = 3284.57 g/mol Now we can calculate the number of moles using the formula: moles = mass/molar mass moles = 49.0 g / 3284.57 g/mol moles = 0.0149 mol At STP (standard temperature and pressure, which is 0°C and 1 atm), one mole of gas occupies 22.4 L of volume. Therefore, the volume of 0.0149 mol of gas at STP can be calculated as: V = nRT/P V = (0.0149 mol)(0.08206 L⋅atm/mol⋅K)(273 K)/(1 atm) V = 0.333 L or 333 mL However, the question asks for the volume of 49.0 g of gas, which is a larger amount than 0.0149 mol. We can use dimensional analysis to convert the volume we just calculated into the volume of 49.0 g of gas: 0.333 L x (49.0 g / 0.0149 mol) = 1092 L (rounded to two significant figures) Therefore, the answer is choice (C), 39 L.

Quiz 11: Gases and Their Properties

A balloon is filled with He gas to a volume of 2.10 L at 35 °C.The balloon is placed in liquid nitrogen until its temperature reaches -196 °C.Assuming the pressure remains constant,what is the volume of the cooled balloon?

What volume of oxygen will react with 21 mL of ethanol,assuming the gases are present at the same temperature and pressure? 2 CH₃CH₂OH(g) + 6 O₂(g) → 4 CO₂(g) + 6 H₂O(g)

A 2.00-L glass soda bottle filled only with air is tightly capped at 19°C and 732.0 mmHg.If the bottle is placed in water at 89°C,what is the pressure in the bottle?

A 26.4-L sample of nitrogen at 7.50 atm and 24°C is simultaneously expanded to 58.4 L and heated to 35°C.What is the new pressure of the gas?

Equal volumes of propane,C₃H₈,and carbon monoxide,CO,at the same temperature and pressure have the same ____.

The pressure of O₂ in a 15.0 L flask is 322 mm Hg at 44 °C.What mass of O₂ is in the flask? (R = 0.08206 L⋅atm/mol⋅K)

The temperature of a specific amount of gas in a sealed container changes from 40.0°C to 80.0°C.If the volume remains constant,the pressure will change from 755 mmHg to ___.

What is the pressure of a 52.5-L gas sample containing 1.57 mol of gas at 93.2°C? (R = 0.0821 L • atm/(K • mol) ,1 atm = 760 mmHg)

What is the final volume of nitrogen gas if the pressure of 5.8 L of the gas is decreased to one-half of its original pressure,and its absolute temperature is increased to double the original temperature?

What volume is occupied by 35.0 g of C₂H₂ at 471 mm Hg and 21 °C? (R = 0.08206 L⋅atm/mol⋅K)

A gas occupying a volume of 1.50 L exerts a pressure of 700 mmHg at 200°C.Which mathematical expression gives the correct pressure at 9.00 L and 350°C?

A 45.0 L gas cylinder contains 988 g He at 23 °C.What is the pressure inside the cylinder? (R = 0.08206 L⋅atm/mol⋅K)

Gaseous chlorine is held in two separate containers at identical temperatures and pressures.The volume of container 1 is 1.30 L,and it contains 6.70 mol of the gas.The volume of container 2 is 2.75 L.How many moles of the gas are in container 2?

If 0.357 g of CH₄ gas is introduced into an empty 1.75 L flask at 25 °C,what will be the pressure inside the flask? (R = 0.08206 L⋅atm/mol⋅K)

You have 34.5 g of O₂ gas in a container with twice the volume as one with CO₂ gas.The pressure and temperature of both containers are the same.Calculate the mass of carbon dioxide gas you have in the container.

Which of the following gases has the greatest density at 35 °C and 450 mm Hg?

The volume of a sample of gas measured at 50.0°C and 1.00 atm pressure is 2.00 L.What must the final temperature be in order for the gas to have a final volume of 3.00 L at 1.00 atm pressure?

What volume of gaseous silane,SiH₄,has the same moles of gas as 9.00 L of helium gas at the same temperature and pressure?

What volume does 49.0 g of N₂ gas occupy at STP? (R = 0.08206 L⋅atm/mol⋅K)

Quiz 11: Gases and Their Properties

A balloon is filled with He gas to a volume of 2.10 L at 35 °C.The balloon is placed in liquid nitrogen until its temperature reaches -196 °C.Assuming the pressure remains constant,what is the volume of the cooled balloon?

What volume of oxygen will react with 21 mL of ethanol,assuming the gases are present at the same temperature and pressure? 2 CH3CH2OH(g) + 6 O2(g) → 4 CO2(g) + 6 H2O(g)

A 2.00-L glass soda bottle filled only with air is tightly capped at 19°C and 732.0 mmHg.If the bottle is placed in water at 89°C,what is the pressure in the bottle?

A 26.4-L sample of nitrogen at 7.50 atm and 24°C is simultaneously expanded to 58.4 L and heated to 35°C.What is the new pressure of the gas?

Equal volumes of propane,C3H8,and carbon monoxide,CO,at the same temperature and pressure have the same ____.

The pressure of O2 in a 15.0 L flask is 322 mm Hg at 44 °C.What mass of O2 is in the flask? (R = 0.08206 L⋅atm/mol⋅K)

The temperature of a specific amount of gas in a sealed container changes from 40.0°C to 80.0°C.If the volume remains constant,the pressure will change from 755 mmHg to ___.

What is the pressure of a 52.5-L gas sample containing 1.57 mol of gas at 93.2°C? (R = 0.0821 L • atm/(K • mol) ,1 atm = 760 mmHg)

What is the final volume of nitrogen gas if the pressure of 5.8 L of the gas is decreased to one-half of its original pressure,and its absolute temperature is increased to double the original temperature?

What volume is occupied by 35.0 g of C2H2 at 471 mm Hg and 21 °C? (R = 0.08206 L⋅atm/mol⋅K)

A gas occupying a volume of 1.50 L exerts a pressure of 700 mmHg at 200°C.Which mathematical expression gives the correct pressure at 9.00 L and 350°C?

A 45.0 L gas cylinder contains 988 g He at 23 °C.What is the pressure inside the cylinder? (R = 0.08206 L⋅atm/mol⋅K)

Gaseous chlorine is held in two separate containers at identical temperatures and pressures.The volume of container 1 is 1.30 L,and it contains 6.70 mol of the gas.The volume of container 2 is 2.75 L.How many moles of the gas are in container 2?

If 0.357 g of CH4 gas is introduced into an empty 1.75 L flask at 25 °C,what will be the pressure inside the flask? (R = 0.08206 L⋅atm/mol⋅K)

You have 34.5 g of O2 gas in a container with twice the volume as one with CO2 gas.The pressure and temperature of both containers are the same.Calculate the mass of carbon dioxide gas you have in the container.

Which of the following gases has the greatest density at 35 °C and 450 mm Hg?

The volume of a sample of gas measured at 50.0°C and 1.00 atm pressure is 2.00 L.What must the final temperature be in order for the gas to have a final volume of 3.00 L at 1.00 atm pressure?

What volume of gaseous silane,SiH4,has the same moles of gas as 9.00 L of helium gas at the same temperature and pressure?

What volume does 49.0 g of N2 gas occupy at STP? (R = 0.08206 L⋅atm/mol⋅K)

What volume of oxygen will react with 21 mL of ethanol,assuming the gases are present at the same temperature and pressure? 2 CH₃CH₂OH(g) + 6 O₂(g) → 4 CO₂(g) + 6 H₂O(g)

Equal volumes of propane,C₃H₈,and carbon monoxide,CO,at the same temperature and pressure have the same ____.

The pressure of O₂ in a 15.0 L flask is 322 mm Hg at 44 °C.What mass of O₂ is in the flask? (R = 0.08206 L⋅atm/mol⋅K)

What volume is occupied by 35.0 g of C₂H₂ at 471 mm Hg and 21 °C? (R = 0.08206 L⋅atm/mol⋅K)

If 0.357 g of CH₄ gas is introduced into an empty 1.75 L flask at 25 °C,what will be the pressure inside the flask? (R = 0.08206 L⋅atm/mol⋅K)

You have 34.5 g of O₂ gas in a container with twice the volume as one with CO₂ gas.The pressure and temperature of both containers are the same.Calculate the mass of carbon dioxide gas you have in the container.

What volume of gaseous silane,SiH₄,has the same moles of gas as 9.00 L of helium gas at the same temperature and pressure?

What volume does 49.0 g of N₂ gas occupy at STP? (R = 0.08206 L⋅atm/mol⋅K)