Calculate the equilibrium constant for the following reaction at 25^$\circ$C 2TiCl₃(s) + 2HCl(g) → 2TiCl₄(g) + H₂(g)
Given $\Delta$ G^$\circ$ = +46.6 kJ.

Question

Calculate the equilibrium constant for the following reaction at 25 $\circ$ C 2TiCl₃(s)+ 2HCl(g) → 2TiCl₄(g)+ H₂(g) Given $\Delta$G $\circ$ = +46.6 kJ.

Quizplus · Accepted Answer

The equilibrium constant (K) can be calculated using the equation: 
K = e^(-ΔG/RT), where ΔG is the change in Gibbs free energy, R is the gas constant, and T is the temperature in Kelvin.

Plugging in the given values, we get:
K = e^(-46.6 kJ/(8.314 J/mol*K * 298 K))
K = 6.7*10^19

Therefore, the best choice is C.

Calculate the Equilibrium Constant for the Following Reaction at 25 ∘\circ∘

Calculate the Equilibrium Constant for the Following Reaction at 25^$\circ$