Question

A 0.316\,\text{mol}0.316mol0, point, 316, start text, m, o, l, end text sample of nitrogen gas, \text{N}_2(g)N

Answer 1

Answer:

2.04 atm

Explanation:

The pressure of the gas can be found by using the equation of state for an ideal gas:

$pV=nRT$

where

p is the gas pressure

V is the gas volume

n is the number of moles

R is the gas constant

T is the absolute temperature of the gas

For this gas we have:

n = 0.316 mol (moles)

V = 4.00 L (volume)

T = 315 K (absolute temperature)

$R=0.082 atm \cdot L/(mol K)$ (gas constant)

Therefore, the gas pressure is

$p=\frac{nRT}{V}=\frac{(0.316)(0.082)(315)}{4.00}=2.04 atm$