ideal gas laws chemisrty

Question

What is the pressure exerted by 5.00 moles of nitrogen gas contained in a 30.0 Liter container at 25.0 °C?

Answer 1

Use the Ideal Gas Law Equation to solve this problem. The Ideal Gas Law equation is:

PV = nRT

P = the pressure (in atm)

V = the volume in L

n = the number of moles of the gas

R = the Gas constant (for this problem it is 0.082057 L*atm/(mol*K) )

T = the temperature in Kelvin

The question wants us to find the pressure, so P = what we want to find. The problem says that the gas is "contained in a 30.0 L container", so V = 30.0 L. The problem says that there are 5.00 moles of nitrogen gas, so n = 5.00. We already established that R = 0.082057 L*atm/(mol*K) for this problem. We need to convert the temperature to Kelvin. To convert Celsius to Kelvin, we use this conversion factor: K = 273.15 + Celsius.

In this problem, Celsius = 25.0, so K = 273.15 + 25.0. So for this problem, the temperature is 298.15 K.

So T = 298.15 K. We put all this information in the Ideal Gas Law equation and solve for P:

PV = nRT

P * 30.0 = 5.00 * 0.082057 * 298.15

P * 30.0 = 122.326473

P = 122.326473 / 30

P = 4.07754909 atm

So the pressure is 4.08 atm.