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
 

If K_p of the reaction $\mathrm{A}\left(\mathrm{g}\right)+2\mathrm{B}\left(\mathrm{g}\right)\rightleftharpoons 3\mathrm{C}\left(\mathrm{g}\right)+\mathrm{D}\left(\mathrm{g}\right)$ is 0.05 at 1000 K, then the value of K_c of the reaction

1. 20000 R

2. 0.02 R

3. $\frac{5\times {10}^{-5}}{\mathrm{R}}$

4. $5\times {10}^{-5}\mathrm{R}$

What will be the change in the concentration of Cl₂ when the equilibrium concentration of PCl₃ is doubled in the reaction:

PCl₅(s) ⇌ PCl₃(g) + Cl₂(g)?

1. Cl₂ becomes half of its initial concentration

2. Cl₂ becomes one-fourth of its initial concentration

3. Cl₂ becomes four times its initial concentration

4. Cl₂ becomes twice its initial concentration