Consider the following reaction.

2NO2(g)⇌N2O4(g)

When the system is at equilibrium, it contains NO2 at a pressure of 0.878 atm , and N2O4 at a pressure of 0.0771 atm . The volume of the container is then reduced to half its original volume. What is the pressure of each gas after equilibrium is reestablished?

Question

28-02-2022
Chemistry

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Consider the following reaction.

2NO2(g)⇌N2O4(g)

When the system is at equilibrium, it contains NO2 at a pressure of 0.878 atm , and N2O4 at a pressure of 0.0771 atm . The volume of the container is then reduced to half its original volume. What is the pressure of each gas after equilibrium is reestablished?

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Oseni Oseni · Answer 1 · 2022-03-09T10:13:43+01:00

The pressure of NO2 and N2O4 would be 1.756 atm and 0.1542 atm respectively.

Gas laws

According to Boyle's law, the pressure of a gas is inversely proportional to its volume at a constant temperature.

Mathematically: P1V1=P2V2

When the volume of a gas is halved at a constant temperature, the pressure is doubled. If it is the volume is doubled, the pressure would be halved.

In this case, the volume of the container is halved. Meaning that the pressure of each of the gas would be doubled by the time the equilibrium is reestablished.

Thus, NO2 would double from 0.878 atm to 1.756 atm while N2O4 will double from 0.0771 atm to 0.1542 atm

More on gas laws can be found here: https://brainly.com/question/1190311