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Question

A closed flask contains NH3 gas at 76 cm of Hg pressure. Now a spark is created due to which, ammonia gas partially dissociates into N2 and H2. 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: 2NH3(g)N2(g)+3H2
Before sparkling
pressure: 76 0 0
After sparkling, when equilibrium is reached,
Pressure: 76-2x x 3x
So, final pressure = 762x+x+3x = 76+2x
Given, Final pressure = 82 cm of Hg
Equating, 82 = 76+2x
We get, x = 3 cm of Hg
Partial pressure of Hydrogen = 9 cm of Hg

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