Equilibrium Test 11

Direction (Q. Nos. 1-9) This section contains 9 multiple choice questions. Each question has four
choices (a), (b), (c) and (d), out of which ONLY ONE option is correct.

Q. For the reaction in equilibrium,
I. CO(g) + 1/2O₂(g)  

II. 2CO(g) + O₂ (g)  2CO₂ (g)
 

Then

Equilibrium constant for the following equilibrium,

is 1.0 x 10²⁸ at a temperature at which RT = 2500 J mol^-1. Gibbs free energy change (ΔG°) is

K_p for the equilibrium  N₂O₄ (g)  2NO₂ (g)  is 0.141 at 25°C and 1 bar. This reaction is spontaneous at 25°C and partial pressures of

For the following equilibrium at 373 K,
H₂O(g)H₂O(g)
ΔAG° is

For the following electrochemical cell reaction at 298 K,
 
E^°cell = 1.10 V

Given 
COCl₂(g)  CO(g) + Cl₂ (g)
Kp = 8 x 10^-9 atm
ΔS° = 30 cal K^-1 at 373 K.
Temperature at which phosgene will be 0.1 % dissociated at 2 atm
(R = 2 cal mol^-1K^-1)is

For the following equilibrium at 298 K,
CO(g) + H₂O (g)  CO₂(g) + H₂(g);
Δ _f G° (in kcal mol^-1) of CO = - 32.81, CO₂ = - 94.26, H₂O = - 54.64, H₂ = 0.0 then, degree of dissociation of CO(g) is

At 1 atmospheric pressure, N₂O₄ is 50% dissociated at 300 K and 80% dissociated at 400 K as given
N₂O₄ (g)  2NO₂ (g)
Thus, enthalpy of dissociation is

At 800 K, ΔG° for the reaction

NiO (s) + H₂(g)  Ni (s) + H₂O (g)

is - 9.0 kcal. Thus, ratio of pressures of water vapours and hydrogen in equilibrium with NiO and Ni at 800 K in terms of logarithm is

Direction (Q. Nos. 10) This sectionis based on statement I and Statement II. Select the correct answer from the code given below.

Q. Statement I

For a reaction  2NO₂(g)  N₂O₄ (g) variation of (log₁₀ K) with (T^-1) is represented as

Statement II

Association o f NO₂ to N₂O₄ is an exotherm ic efiange.