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1 year ago

What is the pressure of 0.5 mol nitrogen (N2) gas in a 5.0 L container at 203 K?

Chemistry

1 answer:

Yuki888 [10]1 year ago

6 0

Answer:

The pressure of 0.5 mole of nitrogen gas= $168.78 k pa$

Given:

Moles of nitrogen gas=0.5mole

Volume of nitrogen gas=5L

Temperature of nitrogen gas=203K

To Find:

Pressure of 0.5g mole of nitrogen gas

Step by Step by Explanation:

Formula used for calculating the pressure of a gas is achieved through ideal gas equation

According to Ideal Gas;

$P V=n R T$

From this above equation, pressure can be calculated as

$P=\frac{n R T}{V}$

Where P=Pressure of the gas

N=number of moles=0.5moles

R=Gas constant $=8.3144598 L k p_{a} k^{-1} m o l^{-1}$

V=Volume of nitrogen gas in litres=5L

T=Temperature of nitrogen gas=203K

Substitute all the values in the above equation we get

$P=\frac{0.5 \times 8.3144598 \times 203}{5}$

$P=\frac{843.9177}{5}$

$P=168.78 k pa$

Result:

Thus the pressure of 0.5 mole of nitrogen gas is $168.78 k pa$

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