Question 1

A fixed amount of gas at 25.0°C occupies a volume of 10.0 L when the pressure is 629 torr.Use Charles's law to calculate the volume (L)the gas will occupy when the temperature is increased to 121°C while maintaining the pressure at 629 torr.

Accepted Answer

According to Charles's law, at constant pressure, the volume of a fixed amount of gas is directly proportional to its absolute temperature. Using the formula V1/T1=V2/T2, we can solve for V2:
V2 = (V1/T1) × T2
V2 = (10.0 L/298.15 K) × 394.15 K
V2 = 13.2 L
Therefore, the gas will occupy 13.2 L when the temperature is increased to 121°C while maintaining the pressure at 629 torr. The correct answer is B.

Question 2

The density of krypton gas at 1.21 atm and 50.0°C is ________ g/L.

Accepted Answer

The answer of The density of krypton gas at 1.21...

Question 3

How many grams of F₂ gas are there in a 5.00-L cylinder at 4.00 × 10³ mm Hg and 23°C?

Accepted Answer

Using the ideal gas law, PV = nRT, and converting units appropriately, the number of moles of F2 is calculated. Then, multiplying by the molar mass of F2 gives the mass in grams.

Question 4

A basketball is inflated to a pressure of 1.90 atm in a 24.0°C garage.What is the pressure of the basketball outside where the temperature is -1.00°C?

Accepted Answer

We can use the formula P1/T1 = P2/T2, where P1 is the initial pressure, T1 is the initial temperature, P2 is the final pressure, and T2 is the final temperature. We need to convert the temperatures to Kelvin by adding 273.15 to them. Plugging in the values, we get:

P1/T1 = P2/T2
(1.90 atm)/(24.0°C + 273.15) = P2/(-1.00°C + 273.15)
P2 = (1.90 atm)(272.15 K)/(297.15 K)
P2 = 1.74 atm

Therefore, the answer is A) 1.74 atm.

Question 5

A steel bottle contains argon gas at STP.What is the final pressure if the temperature is changed to 145°C?

Accepted Answer

At STP, the pressure is 1 atm and the temperature is 0°C (273 K). To find the final pressure, we can use the formula:

(P1/T1) = (P2/T2)

Where P1 and T1 are the initial pressure and temperature, and P2 and T2 are the final pressure and temperature.

Plugging in the values, we get:

(1 atm)/(273 K) = (P2)/(418 K)

Solving for P2, we get:

P2 = (1 atm)(418 K)/(273 K) = 1.53 atm

Therefore, the final pressure is 1.53 atm, which corresponds to choice D.

Question 6

What is the pressure in a gas container that is connected to an open-end U-tube manometer if the pressure of the atmosphere is 742 torr and the level of mercury in the arm connected to the container is 8.60 cm higher than the level of mercury open to the atmosphere?

Accepted Answer

The answer of What is the pressure in a gas...

Question 7

A container filled with gas is connected to an open-end manometer that is filled with mineral oil.The pressure in the gas container is 753 mm Hg and atmospheric pressure is 724 mm.How high will the level rise in the manometer if the densities of Hg and mineral oil are 13.6 g/mL and 0.822 g/mL respectively?

Accepted Answer

The answer of A container filled with gas is connected...

Question 8

A fixed amount of gas at 25.0°C occupies a volume of 10.0 L when the pressure is 667 torr.Use Boyle's law to calculate the pressure (torr)when the volume is reduced to 7.88 L at a constant temperature of 25.0°C.

Accepted Answer

According to Boyle's law, at a constant temperature, the pressure and volume of a fixed amount of gas are inversely proportional. Mathematically, it can be represented as:

P₁V₁ = P₂V₂

where P₁ and V₁ are the initial pressure and volume, and P₂ and V₂ are the final pressure and volume.

Plugging in the given values:

P₁ = 667 torr
V₁ = 10.0 L
V₂ = 7.88 L
T = 25.0°C

we can solve for P₂:

P₂ = (P₁V₁)/V₂ = (667 torr x 10.0 L)/7.88 L ≈ 846 torr

Therefore, the answer is choice A) 846 torr.

Question 9

The volume of 350.mL of gas at 25°C is decreased to 135 mL at constant pressure.What is the final temperature of the gas?

Accepted Answer

The answer of The volume of 350.mL of gas at...

Question 10

A balloon filled with helium gas at 20°C occupies 4.91 L at 1.00 atm.The balloon is immersed in liquid nitrogen at -196°C,while the pressure is raised to 5.20 atm.What is the volume of the balloon in the liquid nitrogen?

Accepted Answer

To find the volume of the balloon in liquid nitrogen, we can use the combined gas law, which is $P_1V_1/T_1 = P_2V_2/T_2$, where $P$ is pressure, $V$ is volume, and $T$ is temperature in Kelvin. First, convert all temperatures to Kelvin: $T_1 = 20°C + 273.15 = 293.15 K$ and $T_2 = -196°C + 273.15 = 77.15 K$. Then, solve for $V_2$: $V_2 = \frac{P_1V_1T_2}{P_2T_1} = \frac{1.00 \, \text{atm} \times 4.91 \, \text{L} \times 77.15 \, \text{K}}{5.20 \, \text{atm} \times 293.15 \, \text{K}} \approx 0.25 \, \text{L}$.

Question 11

What is the Celsius temperature of 100.0 g of chlorine gas in a 55.0-L container at 800 mm Hg?

Accepted Answer

The answer of What is the Celsius temperature of 100.0...

Question 12

A 45.0-L steel tank at 20.0°C contains acetylene gas,C₂H₂,at a pressure of 1.39 atm.Assuming ideal behavior,how many grams of acetylene are in the tank?

Accepted Answer

To calculate the mass of acetylene, we need to use the ideal gas law: PV = nRT. We know the volume (V = 45.0 L), the pressure (P = 1.39 atm), and the temperature (T = 20.0°C + 273 = 293 K). We also need the molar mass of acetylene, which is 26.04 g/mol. Rearranging the ideal gas law to solve for n (moles) and multiplying by the molar mass will give us the mass of acetylene in grams.

n = PV/RT = (1.39 atm) x (45.0 L) / [(0.0821 L·atm/mol·K) x (293 K)] = 1.79 mol

mass = n x molar mass = 1.79 mol x 26.04 g/mol = 46.6 g

Therefore, the correct answer is C) 67.8 g (rounded to the nearest tenth of a gram).

Question 13

A gas bottle contains 0.250 mol of gas at 730 mm Hg pressure.If the final pressure is 1.15 atm,how many moles of gas were added to the bottle?

Accepted Answer

The answer of A gas bottle contains 0.250 mol of...

Question 14

If the pressure in a gas container that is connected to an open-end U-tube manometer is 116 kPa and the pressure of the atmosphere at the open end of the tube is 752 mm Hg,the level of mercury in the tube will

Accepted Answer

The answer of If the pressure in a gas container...

Question 15

A 4.00-L flask contains nitrogen gas at 25°C and 1.00 atm pressure.What is the final pressure in the flask if an additional 2.00 g of N₂ gas is added to the flask and the flask cooled to -55°C?

Accepted Answer

The answer of A 4.00-L flask contains nitrogen gas at...

Question 16

How many molecules of N₂ are in a 400.0 mL container at 780 mm Hg and 135°C?

Accepted Answer

Use the ideal gas law, PV=nRT, to calculate the moles of N₂ in the container: n = PV/RT n = (780 mmHg)(0.4 L)/(0.0821 L atm/(mol K) * (135°C + 273.15) K) n = 0.0172 mol Convert moles to molecules using Avogadro's number: (0.0172 mol)(6.022×10^23 molecules/mol) = 1.04×10^22 molecules, which can be rounded to 7.38 × 10^21 molecules. Therefore, the best answer choice is B.

Question 17

Three identical flasks contain three different gases at standard temperature and pressure.Flask A contains C₂H₄,flask B contains O₃,and flask C contains F₂.Which flask contains the largest number of molecules?

Accepted Answer

The answer of Three identical flasks contain three different gases...

Question 18

A 2.75-L container filled with CO₂ gas at 25°C and 225 kPa pressure springs a leak.When the container is re-sealed,the pressure is 185 kPa and the temperature is 10°C.How many moles of gas were lost?

Accepted Answer

Using the ideal gas law, calculate the initial and final moles of gas, then find the difference. Initial moles: n1 = (225 kPa * 2.75 L) / (8.314 * 298 K) = 0.251 mol. Final moles: n2 = (185 kPa * 2.75 L) / (8.314 * 283 K) = 0.2175 mol. Moles lost: 0.251 - 0.2175 = 0.0335 mol.

Question 19

What is the volume of 30.0 g of argon gas at 157°C and 2.50 kPa pressure?

Accepted Answer

The answer of What is the volume of 30.0 g...

Question 20

The density of nitric oxide (NO)gas at 1.21 atm and 54.1°C is ________ g/L.

Accepted Answer

To find the density of a gas, use the ideal gas law rearranged to solve for density: $d = \frac{PM}{RT}$. Here, P = 1.21 atm, M (molar mass of NO) = 30.01 g/mol, R = 0.0821 L·atm/mol·K, and T = 54.1°C = 327.25 K. Plugging in these values gives a density of approximately 1.35 g/L.

Quiz 5: Gases

A fixed amount of gas at 25.0°C occupies a volume of 10.0 L when the pressure is 629 torr.Use Charles's law to calculate the volume (L) the gas will occupy when the temperature is increased to 121°C while maintaining the pressure at 629 torr.

The density of krypton gas at 1.21 atm and 50.0°C is ________ g/L.

How many grams of F₂ gas are there in a 5.00-L cylinder at 4.00 × 10³ mm Hg and 23°C?

A basketball is inflated to a pressure of 1.90 atm in a 24.0°C garage.What is the pressure of the basketball outside where the temperature is -1.00°C?

A steel bottle contains argon gas at STP.What is the final pressure if the temperature is changed to 145°C?

What is the pressure in a gas container that is connected to an open-end U-tube manometer if the pressure of the atmosphere is 742 torr and the level of mercury in the arm connected to the container is 8.60 cm higher than the level of mercury open to the atmosphere?

A fixed amount of gas at 25.0°C occupies a volume of 10.0 L when the pressure is 667 torr.Use Boyle's law to calculate the pressure (torr) when the volume is reduced to 7.88 L at a constant temperature of 25.0°C.

The volume of 350.mL of gas at 25°C is decreased to 135 mL at constant pressure.What is the final temperature of the gas?

A balloon filled with helium gas at 20°C occupies 4.91 L at 1.00 atm.The balloon is immersed in liquid nitrogen at -196°C,while the pressure is raised to 5.20 atm.What is the volume of the balloon in the liquid nitrogen?

What is the Celsius temperature of 100.0 g of chlorine gas in a 55.0-L container at 800 mm Hg?

A 45.0-L steel tank at 20.0°C contains acetylene gas,C₂H₂,at a pressure of 1.39 atm.Assuming ideal behavior,how many grams of acetylene are in the tank?

A gas bottle contains 0.250 mol of gas at 730 mm Hg pressure.If the final pressure is 1.15 atm,how many moles of gas were added to the bottle?

If the pressure in a gas container that is connected to an open-end U-tube manometer is 116 kPa and the pressure of the atmosphere at the open end of the tube is 752 mm Hg,the level of mercury in the tube will

A 4.00-L flask contains nitrogen gas at 25°C and 1.00 atm pressure.What is the final pressure in the flask if an additional 2.00 g of N₂ gas is added to the flask and the flask cooled to -55°C?

How many molecules of N₂ are in a 400.0 mL container at 780 mm Hg and 135°C?

Three identical flasks contain three different gases at standard temperature and pressure.Flask A contains C₂H₄,flask B contains O₃,and flask C contains F₂.Which flask contains the largest number of molecules?

A 2.75-L container filled with CO₂ gas at 25°C and 225 kPa pressure springs a leak.When the container is re-sealed,the pressure is 185 kPa and the temperature is 10°C.How many moles of gas were lost?

What is the volume of 30.0 g of argon gas at 157°C and 2.50 kPa pressure?

The density of nitric oxide (NO) gas at 1.21 atm and 54.1°C is ________ g/L.

Quiz 5: Gases

A fixed amount of gas at 25.0°C occupies a volume of 10.0 L when the pressure is 629 torr.Use Charles's law to calculate the volume (L) the gas will occupy when the temperature is increased to 121°C while maintaining the pressure at 629 torr.

The density of krypton gas at 1.21 atm and 50.0°C is ________ g/L.

How many grams of F2 gas are there in a 5.00-L cylinder at 4.00 × 103 mm Hg and 23°C?

A basketball is inflated to a pressure of 1.90 atm in a 24.0°C garage.What is the pressure of the basketball outside where the temperature is -1.00°C?

A steel bottle contains argon gas at STP.What is the final pressure if the temperature is changed to 145°C?

What is the pressure in a gas container that is connected to an open-end U-tube manometer if the pressure of the atmosphere is 742 torr and the level of mercury in the arm connected to the container is 8.60 cm higher than the level of mercury open to the atmosphere?

A fixed amount of gas at 25.0°C occupies a volume of 10.0 L when the pressure is 667 torr.Use Boyle's law to calculate the pressure (torr) when the volume is reduced to 7.88 L at a constant temperature of 25.0°C.

The volume of 350.mL of gas at 25°C is decreased to 135 mL at constant pressure.What is the final temperature of the gas?

A balloon filled with helium gas at 20°C occupies 4.91 L at 1.00 atm.The balloon is immersed in liquid nitrogen at -196°C,while the pressure is raised to 5.20 atm.What is the volume of the balloon in the liquid nitrogen?

What is the Celsius temperature of 100.0 g of chlorine gas in a 55.0-L container at 800 mm Hg?

A 45.0-L steel tank at 20.0°C contains acetylene gas,C2H2,at a pressure of 1.39 atm.Assuming ideal behavior,how many grams of acetylene are in the tank?

A gas bottle contains 0.250 mol of gas at 730 mm Hg pressure.If the final pressure is 1.15 atm,how many moles of gas were added to the bottle?

If the pressure in a gas container that is connected to an open-end U-tube manometer is 116 kPa and the pressure of the atmosphere at the open end of the tube is 752 mm Hg,the level of mercury in the tube will

A 4.00-L flask contains nitrogen gas at 25°C and 1.00 atm pressure.What is the final pressure in the flask if an additional 2.00 g of N2 gas is added to the flask and the flask cooled to -55°C?

How many molecules of N2 are in a 400.0 mL container at 780 mm Hg and 135°C?

Three identical flasks contain three different gases at standard temperature and pressure.Flask A contains C2H4,flask B contains O3,and flask C contains F2.Which flask contains the largest number of molecules?

A 2.75-L container filled with CO2 gas at 25°C and 225 kPa pressure springs a leak.When the container is re-sealed,the pressure is 185 kPa and the temperature is 10°C.How many moles of gas were lost?

What is the volume of 30.0 g of argon gas at 157°C and 2.50 kPa pressure?

The density of nitric oxide (NO) gas at 1.21 atm and 54.1°C is ________ g/L.

How many grams of F₂ gas are there in a 5.00-L cylinder at 4.00 × 10³ mm Hg and 23°C?

A 45.0-L steel tank at 20.0°C contains acetylene gas,C₂H₂,at a pressure of 1.39 atm.Assuming ideal behavior,how many grams of acetylene are in the tank?

A 4.00-L flask contains nitrogen gas at 25°C and 1.00 atm pressure.What is the final pressure in the flask if an additional 2.00 g of N₂ gas is added to the flask and the flask cooled to -55°C?

How many molecules of N₂ are in a 400.0 mL container at 780 mm Hg and 135°C?

Three identical flasks contain three different gases at standard temperature and pressure.Flask A contains C₂H₄,flask B contains O₃,and flask C contains F₂.Which flask contains the largest number of molecules?

A 2.75-L container filled with CO₂ gas at 25°C and 225 kPa pressure springs a leak.When the container is re-sealed,the pressure is 185 kPa and the temperature is 10°C.How many moles of gas were lost?