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Dalton's Law of Partial Pressures

A closed flas...

Question

A closed flask contains $N H_{3}$ gas at 76 cm of Hg pressure. Now a spark is created due to which, ammonia gas partially dissociates into $N_{2}$ and $H_{2}$ . The mixture is then allowed to attain same intial temperature, the total pressure of the mixture was found to be 82 cm of Hg. Calculate the partial pressure of hydrogen ( in cm of Hg) in the final mixture.

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Solution

Let the partial pressure of NItrogen gas be x cm of Hg
Reaction: $2 N H_{3} (g) ⇌ N_{2} (g) + 3 H_{2}$
Before sparkling
pressure: 76 0 0
After sparkling, when equilibrium is reached,
Pressure: 76-2x x 3x
So, final pressure = $76 - 2 x + x + 3 x$ = $76 + 2 x$
Given, Final pressure = 82 cm of Hg
Equating, 82 = $76 + 2 x$
We get, x = 3 cm of Hg
Partial pressure of Hydrogen = 9 cm of Hg

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