Gas Calculations

In the ideal gas law, P = ​ (a)   , V = ​ (b)   , n = ​ (c)   ,

R = ​​ (d)   , and T = ​ (e)  

• pressure
• volume
• moles
• gas law constant
• temperature

Solve the following problem:

What is the volume of a balloon if it contains 3.2 moles of helium at a temperature of 20⁰C and 1.2 atm?

• 106.55 K

• 53.3 L

• 293 K

• 64.15 L

Solve the following probem:

What pressure is required to contain 0.23 moles of nitrogen gas in a 4.2 L container at a temperature of 45⁰C?

• 1.43 atm

• 0.048 atm

• 2.49 atm

• 19.32 atm

A gas tank carrying 55L of Cl₂ has a pressure of 2.6atm and a temperature of 289K. How many moles of chlorine gas are in the tank?

• 6.03 mol

• 0.55 mol

• 1.45 mol

• 0.75 mol

Choose the correct set of variables to solve the following problem: What is the volume of a balloon if it contains 3.2 moles of helium at a temperature of 20⁰C and 1.2 atm?

• P = x (unknown), V = 3.2 mol, n = 1.2 atm, T = 20⁰C K

• P = 1.2 atm, V = 3.2 mol, n = 20⁰C, T = x (unknown)

• P = 293 K, V = 3.2 mol, n = x (unknown), T = 1.2 atm

• P = 1.2 atm, V = x (unknown), n = 3.2 mol, T = 293 K

Select the option that has all 5 variables in the correct units

If 22.5 L of nitrogen at 748 mm Hg are compressed to 725 mm Hg at constant temperature, what is the new volume?

• 23.2

• 21.8

• 0.0431

• 0.0459

Calculate the new temperature when 6.00 L at 20.0 °C is compressed to 4.00 L.

• 195

• 0.00512

• 440

• 0.00228

The pressure of a gas is reduced from 1200.0 mm Hg to 850.0 mm Hg as the volume of its container is increased by moving a piston from 85.0 mL to 350.0 mL. What would the final temperature be if the original temperature was 90.0°C?

• 1059

• 124

• 0.016

• 62.4

A sealed container has a pressure of 1.5 atm at 25°C. If the temperature is raised to 125°C, what will be the new pressure?

• 2

• 1.12

• 7.5

• 0.3