In the following reaction, we start with $2 m o l$ of $N_{2}$ and $5 m o l$ of $H_{2}$ exerting a total pressure of $7 a t m$ at a given temperature in a closed vessel. When $50 %$ of $N_{2}$ is converted into $N H_{3}$

$N_{2} {+3H}_{2} \to 2 {NH}_{3}$

Partial pressure of $N H_{3}$ is :

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N 2 g + 3 H 2 g → 2 NH 3 g Initial 2 atm 5 atm 0 Partial pressures Reaction - 1 atm - 3 atm + 2 atm -------------- -------------- -------------- Final values 1 atm 2 atm 2 atm Partial pressure of NH 3 = 2 atm

Chemistry - Ideal Gas Question with Solution | TestHub

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