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.

1. 25.6 × 10⁻²
2. 4.6 × 10⁻⁴
3. 46.6 × 10⁻⁴
4. 16.6 × 10⁻⁸

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

In the reaction, the equilibrium concentrations of PCl₅ and PCl₃ are 0.4 and 0.2 mole/liter respectively. If the value of K_c is 0.5, what is the concentration of Cl₂ in mole/liter?

1. 2.0

2. 1.5

3. 1.0

4. 0.5

4 moles each of SO₂ and O₂ gases are allowed to react to form SO₃ in a closed vessel. At equilibrium, 25% of O₂ is used up. The total number of moles of all the gases at equilibrium is

1. 6.5

2. 7.0

3. 8.0

4. 2.0

For the reversible reaction,

N2(g)+3H2(g)⇌2NH3(g)

At 500°C, the value of K_p is 1.44×10^-5 when partial pressure is measured in atmospheres. The corresponding value of K_c, with concentration in mole L^-1, is

1. 1.44×10^-5(0.082×500)^-2

2. 1.44×10^-5/(8.314×773)^-2

3. 1.44×10^-5(0.082×773)^-2

4. 1.44×10^-5/(0.082×773)^-2

If N₂O₄ is dissociation to 33% and 40% at total pressure P₁ and P₂ atm respectively. The ratio of $\frac{{\mathrm{P}}_1}{{\mathrm{P}}_2}$ is

1. $\frac{8}{5}$

2. $\frac{5}{8}$

3. $\frac{9}{5}$

4. $\frac{5}{9}$