Question

A mixture of gaseous nitrogen and gaseous hydrogen attains equilibrium with gaseous Ammonia according to the reaction 12N2(g)+32H2(g)⇌NH3(ε)It is found that at equilibrium when temperature is 673 K, atmospheric pressure is 100, moles of gaseous nitrogen and gaseous hydrogen are in ratio 1:3 and mole percent of gaseous ammonia is 24. The equilibrium constant Kp for the reaction at the above condition is-

• A. (A) 0.0128 atm-1
• B. (B) 0.1876 atm-1
• C. (C) 0.0186 atm-1
• D. (D) 0.558 atm-1

Answer 1

Answer: (A)

(A) 0.0128 atm-1

Answer 2

Explanation:
12N2(g)+32H2(g)⇌NH3(g)Partial pressure of NH3=24100×100=24.0atmPressure of N2+H2=100−24=76atmPartial pressure ofH2=34×76=57atmPartial pressure of N2=14×76=19atmKp=pNH1pN212p+pH3/2=24(19)12×(57)3/2=244.358×(7.549)3=244.358×430=0.0128atm−1