Question

The values of Kₚ / K for the following reactions at 300 K are respectively : (At 300 K, RT = 24.62 dm³ atm mol⁻¹)

N₂ (g) + O₂ (g) ⇋ 2NO(g)
N₂O₄ (g) ⇋ 2NO₂ (g)
N₂ (g) + 3H₂ (g) ⇋ 2NH₃ (g)

(A) 1,24.62 dm³ mol⁻¹, 1.65 × 10⁻³ dm⁻⁶ atm⁻² mol²
(B) 1,24.62 dm³ atm mol⁻¹, 606.0 dm⁶ atm² mol⁻²
(C) 1,4.1 × 10⁻² dm⁻³ atm⁻¹ mol, 606 dm⁶ atm² mol⁻²

Answer 1

The values of Kp/K for the given reactions at 300K are 0.050, 1.4 × 10^-4, and 3.03 × 10^-8 respectively.

To find the values of Kp/K for the given reactions, we can use the equation Kp = Kc(RT)^Δn, where Δn is the difference in the number of moles of gas on the product side and the reactant side.

Step-by-step explanation:

To find the values of Kp/K for the given reactions, we can start by using the equation Kp = Kc(RT)Δn , where Δn is the difference in the number of moles of gas on the product side and the reactant side.

Let's solve each reaction one by one:

1. N₂(g) + O₂(g) ⇋ 2NO(g)

Δn = (2 - 1) - (1 + 1)

= 0

Kp = Kc(RT)Δn

= 0.050 * (24.62)0

= 0.050

2. N₂O₄(g) ⇋ 2NO₂(g)

Δn = (2 - 1) - (1 + 1)

= -1

Kp = Kc(RT)Δn

= 5.9 × 10-3 * (24.62)-1

= 1.4 × 10-4

3. N₂(g) + 3H₂(g) ⇋ 2NH₃(g)

Δn = (2 - 1) - (1 + 3)

= -1

Kp = Kc(RT)Δn

= 1.3 × 10-6 * (24.62)-1

= 3.03 × 10-8