The K_eq for the equilibrium below is 7.52 × 10^-2 at 480.0 °C. 2Cl₂ (g) + 2H₂O (g) 4HCl (g) + O₂ (g)
What is the value of K_eq at this temperature for the following reaction?
2HCl (g) + O₂ (g) Cl₂ (g) + H₂O (g)

Question

The K_eq for the equilibrium below is 7.52 × 10^-2 at 480.0 °C. 2Cl₂ (g) + 2H₂O (g) The Keq for the equilibrium below is 7.52 × 10-2 at 480.0 °C. 2Cl2 (g) + 2H2O (g) 4HCl (g) + O2 (g) What is the value of Keq at this temperature for the following reaction? 2HCl (g) + O2 (g) Cl2 (g) + H2O (g) A) 13.3 B) 3.65 C) -0.0376 D) 5.66 × 10-3 E) 0.274

The K<sub>eq</sub> for the equilibrium below is 7.52 × 10<sup>-2</sup> at 480.0 °C. 2Cl<sub>2</sub> (g) + 2H<sub>2</sub>O (g) 4HCl (g) + O<sub>2</sub> (g) What is the value of K<sub>eq</sub> at this temperature for the following reaction? 2HCl (g) + O<sub>2</sub> (g) Cl<sub>2</sub> (g) + H<sub>2</sub>O (g) A) 13.3 B) 3.65 C) -0.0376 D) 5.66 × 10<sup>-3</sup> E) 0.274

4HCl (g) + O₂ (g)
What is the value of K_eq at this temperature for the following reaction?
2HCl (g) + The Keq for the equilibrium below is 7.52 × 10-2 at 480.0 °C. 2Cl2 (g) + 2H2O (g) 4HCl (g) + O2 (g) What is the value of Keq at this temperature for the following reaction? 2HCl (g) + O2 (g) Cl2 (g) + H2O (g) A) 13.3 B) 3.65 C) -0.0376 D) 5.66 × 10-3 E) 0.274

O₂ (g)

Cl₂ (g) + H₂O (g)

Quizplus · Accepted Answer

To find the K for the second reaction, we can use the following equation:

K(second reaction) = (K(first reaction))^n

Where n is the stoichiometric coefficient of the product in the second reaction divided by the stoichiometric coefficient of the product in the first reaction. In this case, n = 1/2.

Plugging in the given value for K(first reaction) and n, we get:
K(second reaction) = (7.52 × 10^-12)^(1/2) = 3.65 × 10^-6

Therefore, the answer is B: 3.65.

The Keq for the Equilibrium Below Is 7

The K_eq for the Equilibrium Below Is 7