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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
2
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(g)start text, N, end text, start subscript, 2, end subscript, left parenthesis, g, right parenthesis, is placed in a 4.00\,\text L4.00L4, point, 00, start text, L, end text container at 315\,\text K315K315, start text, K, end text.

Respuesta :

skyluke89

Answer:

2.04 atm

Explanation:

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

[tex]pV=nRT[/tex]

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)

[tex]R=0.082 atm \cdot L/(mol K)[/tex] (gas constant)

Therefore, the gas pressure is

[tex]p=\frac{nRT}{V}=\frac{(0.316)(0.082)(315)}{4.00}=2.04 atm[/tex]

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