For the reaction N 2+3 H 2 leftharpoons 2 NH 3, N 2 and H 2 were taken in the molar ratio of 1: 3. Up to the point of equilibrium 50 % each reactant has been reacted. If total pressure at equilibrium is P. The partial pressure of ammonia would be

Question

For the reaction N 2+3 H 2 leftharpoons 2 NH 3, N 2 and H 2 were taken in the molar ratio of 1: 3. Up to the point of equilibrium 50 % each reactant has been reacted. If total pressure at equilibrium is P. The partial pressure of ammonia would be (A) P / 3 (B) P / 6 (C) P / 4 (D) P / 8

Tardigrade Admin · Accepted Answer

<img class="img-fluid question-image" alt="image" src="https://cdn.tardigrade.in/img/question/chemistry/baef748ecf775eef097147b73eb4e76d-.png" /> Total moles =(1-0.5)+(3-1.5)+1=3 ; P NH 3=(1/3) P

Q. For the reaction $N_{2} + 3 H_{2} ⇌ 2 N H_{3}, N_{2}$ and $H_{2}$ were taken in the molar ratio of $1 : 3$ . Up to the point of equilibrium $50%$ each reactant has been reacted. If total pressure at equilibrium is $P$ . The partial pressure of ammonia would be

$P /3$

$P /6$

$P /4$

$P /8$

Total moles $= (1 - 0.5) + (3 - 1.5) + 1 = 3; P_{N H_{3}} = \frac{1}{3} P$

Q. For the reaction N2​+3H2​⇌2NH3​,N2​ and H2​ were taken in the molar ratio of 1:3. Up to the point of equilibrium 50% each reactant has been reacted. If total pressure at equilibrium is P. The partial pressure of ammonia would be

P/3

P/6

P/4

P/8