Ideal Gas Law

PV=nRT

• Charles Law     

• Boyles Law

• Ideal Gas Law 

• Combined Gas Law

Calculate the volume that a 0.323-mol sample of a gas will occupy at 265 K and a pressure of 0.900 atm.

• 7.18 L

• 7.81 L

• 4.63 L

• 4.36 L

There are 65 liters of helium in a balloon at 35 K. If the temperature of the balloon is increased to 40 K, what will the new volume of the balloon be?

• 40 L

• 70 L

• 74.3 L

• 75.9 L

• correct answer is not given

A gas in a metal container at 5 atm (P1) has its temperature changed from 20 K (T1) to 90 K (T2). What is the final pressure in atmospheres (P2)?

• 22.5 atm

• 22.5 K

• 225 atm

• 225K

• correct answer is not given

Choose the correct set of variables to solve the following problem: At what temperature would 4.0 moles of hydrogen gas in a 100 liter container exert a pressure of 1.00 atmospheres?

• P = x (unknown), V = 1.0 atm, n = 100 L, R = 8.314 L·kPa/mol·K, T = 4.0 mol

• P = 100 L, V = 4.00 mol, n = x (unknown), R = 0.0821 L·atm/mol·K, T = 1.00 atm

• P = 4.00 mol, V = x (unknown) , n = 1.0 atm, R = 8.314 L·kPa/mol·K, T = 100 K

• P = 1.00 atm, V = 100 L , n = 4.0 mol, R = 0.0821 L·atm/mol·K, T = x (unknown)

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

• V

• n

• T

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 20⁰C?

• 1.32 atm

• 0.048 atm

• 2.49 atm

• 19.32 atm

Which of the following equations represents the Ideal Gas Law?

A sample of gas occupies 10.0 L at a pressure of 2.0 atm. If the pressure is increased to 4.0 atm while the temperature remains constant, what will be the new volume of the gas?

• 5.0 L

• 20.0 L

• 10.0 L

• 2.5 L