What pressure is requred to contain 0.023 moles of nitrogen gas in a 4.2 L container at a temperature of 20.°C?

0.13 atm

Explanation:

Using the Ideal Gas Law; PV=nRT, we can rearrange to solve for pressure.

P=nRT/V

P is pressure, n is number of moles (0.023), R is a constant (0.08206 L*atm/mol*K), T is temperature in Kelvin (293.15K) and V is volume, 4.2 L.

So, plugging in;

P=(0.023mol)(0.08206L*atm/mol*K)(293.15K)/(4.2 L)

P=0.1317 atm

P=0.13 atm; multiply by 760 to get to Torr or mmHg.

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