Ideal Gas Law (PV=nRT) Example Problem

In this video we’ll work a practice problem for the Ideal Gas Law, PV=nRT. For this problem you can rearrange the equation to get V by itself to start with or just plug in values and solve for V.

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We can determine the volume occupied by 2.34 grams of CO2 gas at 27.2°C and 2.2 atm using the ideal gas law:

PV = nRT

where:

P is the pressure (in atm)
V is the volume (in L)
n is the number of moles of gas
R is the ideal gas constant (0.08206 L atm/mol K)
T is the temperature (in K)

Steps to solve:

Convert the temperature to Kelvin: T = 27.2°C + 273.15 K = 300.35 K

Calculate the number of moles of CO2: n = mass / molar mass = 2.34 g / 44.01 g/mol = 0.0532 mol
Apply the ideal gas law: V = nRT / P = (0.0532 mol)(0.08206 L atm/mol K)(300.35 K) / 2.2 atm ≈ 0.59 L

Therefore, the volume occupied by 2.34 grams of CO2 gas at 27.2°C and 2.2 atm is approximately 0.59 liters.

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