For the reaction, $\mathrm{A}+\mathrm{B}\rightleftharpoons \mathrm{C}+\mathrm{D}$, the rate constants for the forward and backward reactions are found to be $4.2\times {10}^{-2}$ and $3.36\times {10}^{-3}<mspace\; width="1em"></mspace>\mathrm{mol}<mspace\; width="1em"></mspace>{\mathrm{L}}^{-1}<mspace\; width="1em"></mspace>{\mathrm{s}}^{-1}$ respectively. What is the equilibrium constant for the reaction?

1. 11.5

2. 12.5

3. 8.0

4. 6.0

In the reaction $2{\mathrm{H}}_2\mathrm{S}\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{H}}_2\left(\mathrm{g}\right)+{\mathrm{S}}_2\left(\mathrm{g}\right)$ the concentration of H₂S is 0.5 mol L^-1 and concentration of H₂ is 0.1 mol L^-1 while concentration of S₂ is 0.4 mol L^-1 in one litre vessel. The value of equilibrium constant of the reaction is

1. 0.016

2. 0.013

3. 0.020

4. 0.030

For a gaseous reaction ,$2\mathrm{A}+\mathrm{B}\rightleftharpoons \mathrm{C}+\mathrm{D},$

the partial pressure of A, B, C and D at equilibrium are 0.5, 0.8, 0.7 and 1.2 atm. The value of K_p for this reaction is

1. 2.4 atm

2. 6.2 atm^-2

3. 4.2 atm^-1

4. 8.4 atm^-3

For the reaction $\mathrm{C}\left(\mathrm{s}\right)+{\mathrm{CO}}_2\left(\mathrm{g}\right)\rightleftharpoons 2\mathrm{CO}\left(\mathrm{g}\right),$ the partial pressure of CO₂ and CO are 4 and 8 atm respectively. The value of K_p for this reaction is

1. 14 atm

2. 16 atm

3. 18 atm

4. 12 atm

In which of the following gaseous reaction, K_p and K_c have the same values?

1. $2\mathrm{HI}\rightleftharpoons {\mathrm{H}}_2+{\mathrm{I}}_2$

2. ${\mathrm{N}}_2+3{\mathrm{H}}_2\rightleftharpoons 2{\mathrm{NH}}_3$

3. $2{\mathrm{SO}}_2+{\mathrm{O}}_2\rightleftharpoons 2{\mathrm{SO}}_3$

4. ${\mathrm{PCI}}_5\rightleftharpoons {\mathrm{PCII}}_3+{\mathrm{Cl}}_2$

Find the gaseous equilibrium for which Kp < Kc.

Find the value of Kp for the reaction:

N₂(g) + 3H₂(g) ⇌ 2NH₃(g)

Given: Kc = 0.5 at 400 K and R = 0.0821 L atm mol⁻¹ K⁻¹.

Find the value of Kc for the reaction:

2SO₂(g) + O₂(g) ⇌ 2SO₃(g)

at 700 K, if

Kₚ = 1.3 × 10⁻³ atm⁻¹

Find the ratio Kp/Kc for the reaction:

SO₂(g) + ½O₂(g) ⇌ SO₃(g)

1. (RT)^1/2 

2. (RT)^-1/2 

3. (RT)

4. 1

Find the equilibrium constant Kc for the reaction:

½N₂(g) + ½O₂(g) + ½Br₂(g) ⇌ NOBr(g)

Given:

2NO(g) ⇌ N₂(g) + O₂(g)  Kc₁ = 2.5 × 10³⁰

NO(g) + ½Br₂(g) ⇌ NOBr(g)  Kc₂ = 1.6