Given the following chemical equilibrium COCl₂(g) CO(g)+ Cl₂(g),calculate the value of K_cwhen K_p = 6.5 × 10¹¹ at 298 K.(R = 0.08206 L⋅atm/mol ⋅ K)

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The equilibrium constant expression is given as: K_c = [CO][Cl₂]/[COCl₂] We can use the following relation to find K_c from KP: KP = K_c(RT)Δn where Δn = (number of moles of products) - (number of moles of reactants) From the balanced equation, we can see that Δn = 1 - 2 = -1. Substituting the given values and solving for K_c: 6.5 × 10¹¹ = K_c(0.08206 L⋅atm/mol ⋅ K)(298 K)(-1) K_c = 2.74 × 10¹⁰ The closest option is D, 2.7 × 10¹⁰.

Given the Following Chemical Equilibrium COCl2(g) CO(g)+ Cl2(g),calculate the Value

Given the Following Chemical Equilibrium COCl₂(g) CO(g)+ Cl₂(g),calculate the Value