Ideal Gas Law Math

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

What pressure, in kPa, is required to contain 0.23 moles of nitrogen gas in a 4.2 L container at a temperature of 20⁰C?

• P = x (unknown), V = 4.2 L, n = 0.23 mol, R = 8.314 L·kPa/mol·K, T = 293 K

• P = 4.2 L, V = 0.23 mol, n = x (unknown), R = 8.314 L·kPa/mol·K, T = 20⁰C

• P = 0.23 mol, V = x (unknown), n = 293 K, R = 0.0821 L·atm/mol·K, T = 4.2 L

• P = 20⁰C, V = 4.2 L , n = 0.23 mol, R = 0.0821 L·atm/mol·K, T =x (unknown)

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)

We use three R values: 0.0821, 62.4 and 8.314. How do you know which to use for a problem?

• The units for pressure

• The units for temperature

• The units of volume

• The amount of moles

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?

• 0.0821 L⋅atm∕mol⋅K

• 8.314 L⋅kPa∕mol⋅K

• 293 K

• 62.4 L mmHg/mol K

Which of the following variables is NOT correctly matched with its value for this problem: What pressure is required to contain 0.023 moles of nitrogen gas in a 4.2 L container at a temperature of 20⁰C?

• V = 4.2 L

• R = 0.0821 L⋅atm∕mol⋅K

• n = 0.023 mol

• P = 20⁰C

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

What is the correct value for T in the following problem: What pressure is required to contain 0.023 moles of nitrogen gas in a 4.2 L container at a temperature of 20⁰C?

• T = 0.23 K

• T = 293 K

• T = 4.2⁰C

• T = 20⁰C

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