Question 1

A sample of ammonia gas at 65.5$\degree$C and 524 torr has a volume of 15.31 L. What is its volume when the temperature is -15.8$\degree$C and its pressure is 524 torr?

Accepted Answer

This is a combined gas law problem. We can use the equation:

(P1V1/T1) = (P2V2/T2)

Where P1, V1, and T1 are the initial pressure, volume, and temperature, and P2 is the final pressure (which is the same as the initial pressure) and T2 is the final temperature.

Plugging in the given values, we get:

(524 torr)(15.31 L)/(338.5 K) = (524 torr)(V2)/257.4 K

Simplifying, we get:

V2 = (524 torr)(15.31 L)(257.4 K)/(338.5 K)(524 torr)

V2 = 11.6 L

Therefore, the answer is B, 11.6 L.

Question 2

A sample container of carbon monoxide occupies a volume of 435 mL at a pressure of 785 torr and a temperature of 298 K. What would its temperature be if the volume were changed to 265 mL at a pressure of 785 torr?

Accepted Answer

Since the pressure and the amount of gas remain constant, the relationship between volume and temperature can be described by Charles's Law (V1/T1 = V2/T2). Solving for T2 gives T2 = (V2 * T1) / V1. Substituting the given values (V1 = 435 mL, T1 = 298 K, V2 = 265 mL) into the equation yields T2 = (265 mL * 298 K) / 435 mL = 182 K.

Question 3

What are the conditions of STP?

Accepted Answer

STP stands for Standard Temperature and Pressure. It is defined as 273.15 K (0 degrees Celsius) and 760 torr (or 1 atmosphere) of pressure. Therefore, the correct option is B, as it satisfies both the temperature and pressure conditions of STP.

Question 4

A 750-mL sample of hydrogen exerts a pressure of 822 torr at 325 K. What pressure does it exert if the temperature is raised to 475 K at constant volume?

Accepted Answer

We can use the equation for the combined gas law, which states that:

(P1V1)/T1 = (P2V2)/T2

We know that V1 = V2 since the volume is constant, and we can rearrange the equation to solve for P2:

P2 = (P1*T2)/T1

Plugging in the given values, we get:

P2 = (822 torr * 475 K) / 325 K = 1200 torr or 1.20 × 10^3 torr

Therefore, the answer is D.

Question 5

A sample of methane gas, CH₄(g), occupies a volume of 60.3 L at a pressure of 469 torr and a temperature of 29.3$\degree$C. What would be its temperature at a pressure of 243 torr and volume of 60.3 L?

Accepted Answer

We can use the combined gas law to solve the problem: 
P1V1/T1 = P2V2/T2 
where P1, V1, and T1 are the initial pressure, volume, and temperature, respectively, and P2 and V2 are the new pressure and volume, respectively, that we want to find. Rearranging the equation, we get: 
T2 = T1 * P2 * V1 / (P1 * V2)

Plugging in the values, we get: 
T2 = 29.3F1F1F1S1F1F1F10C * 243 torr * 60.3 L / (469 torr * 60.3 L) = -116.5F1F1F1S1F1F1F10C

Note that the temperature is negative, which means that the gas has cooled down. Therefore, the correct answer is (A).

Question 6

Calculate the pressure of a helium sample at -207.3$\degree$C and 768 mL if it exerts a pressure of 175 kPa at 25.0$\degree$C and 925 mL.

Accepted Answer

The answer of Calculate the pressure of a helium sample...

Question 7

A sample of oxygen gas has its absolute temperature halved while the pressure of the gas remained constant. If the initial volume is 400 mL, what is the final volume?

Accepted Answer

According to the Combined Gas Law, when pressure remains constant, if temperature is halved, volume will also be halved. Therefore, the final volume will be 200 mL.

Question 8

A sample of nitrogen gas is confined to a 14.0 L container at 375 torr and 37.0$\degree$C. How many moles of nitrogen are in the container?

Accepted Answer

To find the number of moles of nitrogen gas, use the ideal gas law: PV = nRT. Convert pressure to atm (375 torr = 0.493 atm) and temperature to Kelvin (37°C = 310 K). Using R = 0.0821 L·atm/mol·K, solve for n: n = PV/RT = (0.493 atm)(14.0 L) / (0.0821 L·atm/mol·K)(310 K) ≈ 0.271 mol.

Question 9

A sample of the inert gas krypton has its pressure tripled while its temperature remained constant. If the original volume is 12 L, what is the final volume?

Accepted Answer

According to Boyle's Law (P1V1 = P2V2), if the pressure of a gas is tripled (P2 = 3P1) while the temperature remains constant, the volume of the gas will decrease to a third of its original volume. Therefore, the final volume is 12 L / 3 = 4.0 L.

Question 10

A carbon dioxide sample weighing 44.0 g occupies 32.68 L at 65$\degree$C and 645 torr. What is its volume at STP?

Accepted Answer

The volume of a gas at STP (0°C and 1 atm) can be calculated using the ideal gas law. First, convert the given conditions to STP using the combined gas law: $ V_1/T_1 \times P_1 = V_2/T_2 \times P_2 $. Solving for $ V_2 $ at STP gives approximately 22.4 L.

Question 11

A 0.850-mole sample of nitrous oxide, a gas used as an anesthetic by dentists, has a volume of 20.46 L at 123$\degree$C and 1.35 atm. What would be its volume at 468$\degree$C and 1.35 atm?

Accepted Answer

Using Charles's Law (V1/T1 = V2/T2) and converting temperatures to Kelvin, the initial volume is 20.46 L at 396 K, and the final temperature is 741 K. Solving for V2 gives approximately 38.3 L.

Question 12

A weather balloon was initially at a pressure of 0.950 atm, and its volume was 35.0 L. The pressure decreased to 0.750 atm, without loss of gas or change in temperature. What was the change in the volume?

Accepted Answer

The answer of A weather balloon was initially at a...

Question 13

Calculate the temperature of an argon sample at 55.4 kPa and 18.6 L if it occupies 25.8 L at 75.0$\degree$C and 41.1 kPa.

Accepted Answer

The answer of Calculate the temperature of an argon sample...

Question 14

Which of the lines on the figure below is the best representation of the relationship between the volume and the number of moles of a gas, measured at constant temperature and pressure?

Accepted Answer

The answer of Which of the lines on the figure...

Question 15

A sample of nitrogen gas at 298 K and 745 torr has a volume of 37.42 L. What volume will it occupy if the pressure is increased to 894 torr at constant temperature?

Accepted Answer

The answer of A sample of nitrogen gas at 298...

Question 16

Nitrogen dioxide is a red-brown gas that is responsible for the color of photochemical smog. A sample of nitrogen dioxide has a volume of 28.6 L at 45.3$\degree$C and 89.9 kPa. What is its volume at STP?

Accepted Answer

To solve the problem, we need to use the combined gas law, which relates the pressure, volume, and temperature of a gas. The formula is:

(P1V1/T1) = (P2V2/T2)

where P1, V1, and T1 are the initial conditions, and P2, V2, and T2 are the final conditions.

We are given the initial volume (V1) as 28.6 L, the initial temperature (T1) as 45.3°F = 7.4°C = 280.4 K, and the initial pressure (P1) as 89.9 kPa.

At STP, the temperature is 0°C = 273.15 K, and the pressure is 1 atm = 101.325 kPa.

So, we can plug in these values and solve for V2:

(89.9 kPa × 28.6 L) / 280.4 K = (101.325 kPa × V2) / 273.15 K

V2 = (89.9 kPa × 28.6 L × 273.15 K) / (280.4 K × 101.325 kPa)

V2 = 21.8 L

Therefore, the answer is choice A: 21.8 L.

Question 17

A 500-mL sample of argon at 800 torr has its absolute temperature quadrupled. If the volume remains unchanged what is the new pressure?

Accepted Answer

The answer of A 500-mL sample of argon at 800...

Question 18

A sample of carbon dioxide gas at 125$\degree$C and 248 torr occupies a volume of 275 L. What will the gas pressure be if the volume is increased to 321 L at 125$\degree$C?

Accepted Answer

According to Boyle's Law, which states that pressure and volume are inversely proportional at constant temperature, $ P_1V_1 = P_2V_2 $. Given $ P_1 = 248 $ torr, $ V_1 = 275 $ L, and $ V_2 = 321 $ L, we can solve for $ P_2 $: $ P_2 = \frac{P_1V_1}{V_2} = \frac{248 \times 275}{321} \approx 212 $ torr.

Question 19

A sample of propane, a component of LP gas, has a volume of 35.3 L at 315 K and 922 torr. What is its volume at STP?

Accepted Answer

The answer of A sample of propane, a component of...

Question 20

A sample of an ideal gas has its volume doubled while its temperature remains constant. If the original pressure was 100 torr, what is the new pressure?

Accepted Answer

According to the ideal gas law, PV=nRT, if temperature remains constant (T is constant), then P and V are inversely proportional (P ∝ 1/V). When the volume is doubled (V becomes 2V), the pressure will be halved (P becomes P/2) to maintain the constant temperature. Therefore, the new pressure is 100 torr/2 = 50 torr.

Quiz 5: Gases and the Kinetic-Molecular Theory

A sample of ammonia gas at 65.5 $\degree$ C and 524 torr has a volume of 15.31 L. What is its volume when the temperature is -15.8 $\degree$ C and its pressure is 524 torr?

A sample container of carbon monoxide occupies a volume of 435 mL at a pressure of 785 torr and a temperature of 298 K. What would its temperature be if the volume were changed to 265 mL at a pressure of 785 torr?

What are the conditions of STP?

A 750-mL sample of hydrogen exerts a pressure of 822 torr at 325 K. What pressure does it exert if the temperature is raised to 475 K at constant volume?

A sample of methane gas, CH₄(g) , occupies a volume of 60.3 L at a pressure of 469 torr and a temperature of 29.3 $\degree$ C. What would be its temperature at a pressure of 243 torr and volume of 60.3 L?

Calculate the pressure of a helium sample at -207.3 $\degree$ C and 768 mL if it exerts a pressure of 175 kPa at 25.0 $\degree$ C and 925 mL.

A sample of oxygen gas has its absolute temperature halved while the pressure of the gas remained constant. If the initial volume is 400 mL, what is the final volume?

A sample of nitrogen gas is confined to a 14.0 L container at 375 torr and 37.0 $\degree$ C. How many moles of nitrogen are in the container?

A sample of the inert gas krypton has its pressure tripled while its temperature remained constant. If the original volume is 12 L, what is the final volume?

A carbon dioxide sample weighing 44.0 g occupies 32.68 L at 65 $\degree$ C and 645 torr. What is its volume at STP?

A 0.850-mole sample of nitrous oxide, a gas used as an anesthetic by dentists, has a volume of 20.46 L at 123 $\degree$ C and 1.35 atm. What would be its volume at 468 $\degree$ C and 1.35 atm?

A weather balloon was initially at a pressure of 0.950 atm, and its volume was 35.0 L. The pressure decreased to 0.750 atm, without loss of gas or change in temperature. What was the change in the volume?

Calculate the temperature of an argon sample at 55.4 kPa and 18.6 L if it occupies 25.8 L at 75.0 $\degree$ C and 41.1 kPa.

Which of the lines on the figure below is the best representation of the relationship between the volume and the number of moles of a gas, measured at constant temperature and pressure?

A sample of nitrogen gas at 298 K and 745 torr has a volume of 37.42 L. What volume will it occupy if the pressure is increased to 894 torr at constant temperature?

Nitrogen dioxide is a red-brown gas that is responsible for the color of photochemical smog. A sample of nitrogen dioxide has a volume of 28.6 L at 45.3 $\degree$ C and 89.9 kPa. What is its volume at STP?

A 500-mL sample of argon at 800 torr has its absolute temperature quadrupled. If the volume remains unchanged what is the new pressure?

A sample of carbon dioxide gas at 125 $\degree$ C and 248 torr occupies a volume of 275 L. What will the gas pressure be if the volume is increased to 321 L at 125 $\degree$ C?

A sample of propane, a component of LP gas, has a volume of 35.3 L at 315 K and 922 torr. What is its volume at STP?

A sample of an ideal gas has its volume doubled while its temperature remains constant. If the original pressure was 100 torr, what is the new pressure?

Quiz 5: Gases and the Kinetic-Molecular Theory

A sample of ammonia gas at 65.5 °\degree° C and 524 torr has a volume of 15.31 L. What is its volume when the temperature is -15.8 °\degree° C and its pressure is 524 torr?

A sample container of carbon monoxide occupies a volume of 435 mL at a pressure of 785 torr and a temperature of 298 K. What would its temperature be if the volume were changed to 265 mL at a pressure of 785 torr?

What are the conditions of STP?

A 750-mL sample of hydrogen exerts a pressure of 822 torr at 325 K. What pressure does it exert if the temperature is raised to 475 K at constant volume?

A sample of methane gas, CH4(g) , occupies a volume of 60.3 L at a pressure of 469 torr and a temperature of 29.3 °\degree° C. What would be its temperature at a pressure of 243 torr and volume of 60.3 L?

Calculate the pressure of a helium sample at -207.3 °\degree° C and 768 mL if it exerts a pressure of 175 kPa at 25.0 °\degree° C and 925 mL.

A sample of oxygen gas has its absolute temperature halved while the pressure of the gas remained constant. If the initial volume is 400 mL, what is the final volume?

A sample of nitrogen gas is confined to a 14.0 L container at 375 torr and 37.0 °\degree° C. How many moles of nitrogen are in the container?

A sample of the inert gas krypton has its pressure tripled while its temperature remained constant. If the original volume is 12 L, what is the final volume?

A carbon dioxide sample weighing 44.0 g occupies 32.68 L at 65 °\degree° C and 645 torr. What is its volume at STP?

A 0.850-mole sample of nitrous oxide, a gas used as an anesthetic by dentists, has a volume of 20.46 L at 123 °\degree° C and 1.35 atm. What would be its volume at 468 °\degree° C and 1.35 atm?

A weather balloon was initially at a pressure of 0.950 atm, and its volume was 35.0 L. The pressure decreased to 0.750 atm, without loss of gas or change in temperature. What was the change in the volume?

Calculate the temperature of an argon sample at 55.4 kPa and 18.6 L if it occupies 25.8 L at 75.0 °\degree° C and 41.1 kPa.

Which of the lines on the figure below is the best representation of the relationship between the volume and the number of moles of a gas, measured at constant temperature and pressure?

A sample of nitrogen gas at 298 K and 745 torr has a volume of 37.42 L. What volume will it occupy if the pressure is increased to 894 torr at constant temperature?

Nitrogen dioxide is a red-brown gas that is responsible for the color of photochemical smog. A sample of nitrogen dioxide has a volume of 28.6 L at 45.3 °\degree° C and 89.9 kPa. What is its volume at STP?

A 500-mL sample of argon at 800 torr has its absolute temperature quadrupled. If the volume remains unchanged what is the new pressure?

A sample of carbon dioxide gas at 125 °\degree° C and 248 torr occupies a volume of 275 L. What will the gas pressure be if the volume is increased to 321 L at 125 °\degree° C?

A sample of propane, a component of LP gas, has a volume of 35.3 L at 315 K and 922 torr. What is its volume at STP?

A sample of an ideal gas has its volume doubled while its temperature remains constant. If the original pressure was 100 torr, what is the new pressure?

A sample of ammonia gas at 65.5 $\degree$ C and 524 torr has a volume of 15.31 L. What is its volume when the temperature is -15.8 $\degree$ C and its pressure is 524 torr?

A sample of methane gas, CH₄(g) , occupies a volume of 60.3 L at a pressure of 469 torr and a temperature of 29.3 $\degree$ C. What would be its temperature at a pressure of 243 torr and volume of 60.3 L?

Calculate the pressure of a helium sample at -207.3 $\degree$ C and 768 mL if it exerts a pressure of 175 kPa at 25.0 $\degree$ C and 925 mL.

A sample of nitrogen gas is confined to a 14.0 L container at 375 torr and 37.0 $\degree$ C. How many moles of nitrogen are in the container?

A carbon dioxide sample weighing 44.0 g occupies 32.68 L at 65 $\degree$ C and 645 torr. What is its volume at STP?

A 0.850-mole sample of nitrous oxide, a gas used as an anesthetic by dentists, has a volume of 20.46 L at 123 $\degree$ C and 1.35 atm. What would be its volume at 468 $\degree$ C and 1.35 atm?

Calculate the temperature of an argon sample at 55.4 kPa and 18.6 L if it occupies 25.8 L at 75.0 $\degree$ C and 41.1 kPa.

Nitrogen dioxide is a red-brown gas that is responsible for the color of photochemical smog. A sample of nitrogen dioxide has a volume of 28.6 L at 45.3 $\degree$ C and 89.9 kPa. What is its volume at STP?

A sample of carbon dioxide gas at 125 $\degree$ C and 248 torr occupies a volume of 275 L. What will the gas pressure be if the volume is increased to 321 L at 125 $\degree$ C?