Question

consider the chemical equation and equilibrium constant at 25 ∘c : 2cof2(g)⇌co2(g) cf4(g) , k=2.2×106 calculate the equilibrium constant for the following reaction at 25 ∘c : 2co2(g) 2cf4(g)⇌4cof2(g)

Answer 1

To find the equilibrium constant for the new reaction, the equilibrium constant for the given reverse reaction is squared and then its inverse is taken, resulting in an equilibrium constant of approximately 2.06 x 10^-13.

Step-by-step explanation:

To solve for the equilibrium constant for the reaction 2CO2(g) + 2CF4(g) ⇌ 4COF2(g), first consider the given equilibrium for the reverse reaction, 2COF2(g) ⇌ CO2(g) + CF4(g), with K = 2.2 × 106.

For the reverse reaction, if we double the amounts of substances according to the stoichiometry provided, we would square the equilibrium constant, and since reversing the reaction would be the inverse of the equilibrium constant, the relationship would be:

Knew = 1 / Koriginal2

Thus, we can calculate:

Knew = 1 / (2.2 × 106)2 ≈ 2.06 × 10-13

Answer 2

To calculate the equilibrium constant for a reverse reaction, we simply take the reciprocal of the given equilibrium constant of the forward reaction. For 2 CO2(g) + 2 CF4(g) ⇔ 4 COF2(g) at 25 °C, the equilibrium constant is 4.55 × 10⁻⁷.

Step-by-step explanation:

The original reaction is 2 COF2(g) ⇔ CO2(g) + CF4(g), with an equilibrium constant K = 2.2 × 106 at 25 °C. To calculate the equilibrium constant for the reverse reaction which is:

2 CO2(g) + 2 CF4(g) ⇔ 4 COF2(g),

we just take the reciprocal of the given K, because the reverse reaction has the inverse equilibrium expression. Thus, the equilibrium constant for the reverse reaction is:

K' = 1/K = 1/(2.2 × 106)

Therefore, K' for the reverse reaction at 25 °C is 4.55 × 10-7.