Liquid nitrogen trichloride is heated in a 1.25-L closed reaction vessel until it decomposes completely to gaseous elements. The resulting mixture exerts a pressure of 773 mmHg at 86°C. What is the partial pressure of each gas in the container?

Question

Chemistry

Paris Acosta

27 June, 13:10

Liquid nitrogen trichloride is heated in a 1.25-L closed reaction vessel until it decomposes completely to gaseous elements. The resulting mixture exerts a pressure of 773 mmHg at 86°C. What is the partial pressure of each gas in the container?

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Answers (1)

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Jaydin Garrison · Answer 1

N2 = 193.25mmHg

Cl2 = 579.75mmHg

Explanation:

Total number of moles=4

For N2 mole fraction=1/4

Partial pressure of N2 = 1/4 * 773 = 193.25mmHg

For Cl2, mole fraction = 3/4

Partial pressure of Cl2 = 3/4 * 773 = 579.75 mmHg