Given the equilibrium constant for the following reaction,
H₂(g) + Cl₂(g) 2 HCl(g) K_p = 2.5 x 10⁴
If equimolar amounts of H₂ and Cl₂ are allowed to reach equilibrium in a system in which no HCl was present initially, the ratio of the partial pressures of H₂ to Cl₂ at equilibrium will be

Question

Given the equilibrium constant for the following reaction,
H₂(g) + Cl₂(g)

Given the equilibrium constant for the following reaction, H<sub>2</sub>(g) + Cl<sub>2</sub>(g) 2 HCl(g) K<sub>p</sub> = 2.5 x 10<sup>4</sup> If equimolar amounts of H<sub>2</sub> and Cl<sub>2</sub> are allowed to reach equilibrium in a system in which no HCl was present initially, the ratio of the partial pressures of H<sub>2</sub> to Cl<sub>2</sub> at equilibrium will be A) larger than 1. B) smaller than 1. C) equal to 1. D) a value that can't be generalized by any of the above statements.

2 HCl(g) K_p = 2.5 x 10⁴
If equimolar amounts of H₂ and Cl₂ are allowed to reach equilibrium in a system in which no HCl was present initially, the ratio of the partial pressures of H₂ to Cl₂ at equilibrium will be

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The Answer of Given the equilibrium constant for the following reaction, H₂(g) + Cl₂(g) 2 HCl(g) K_p = 2.5 x 10⁴ If equimolar amounts of H₂ and Cl₂ are allowed to reach equilibrium in a system in which no HCl was present initially, the ratio of the partial pressures of H₂ to Cl₂ at equilibrium will be

Given the Equilibrium Constant for the Following Reaction