In the reaction below, 3.46 atm each of H2 and Cl2 were placed into a 1.00 L flask and allowed to react: H2 (g) + Cl2 (g) 2 HCl (g) Given that Kc = 50.1, calculate the equilibrium pressure of HCl. Enter your answer to 2 decimal places.

Question

Kadence Parker

Chemistry

23 October, 14:14

In the reaction below, 3.46 atm each of H2 and Cl2 were placed into a 1.00 L flask and allowed to react: H2 (g) + Cl2 (g) 2 HCl (g) Given that Kc = 50.1, calculate the equilibrium pressure of HCl. Enter your answer to 2 decimal places.

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Answers (1)

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Amira Roy · Answer 1

The equilibrium pressure of HCl is 5.40 atm

Explanation:

Kc = [HCl]^2/[H2][Cl2]

Initial pressure of H2 = 3.46 atm and Cl2 = 3.46 atm

Let the equilibrium pressure of HCl be y

From the equation of reaction, mole ratio of H2 to HCl is 1:2, equilibrium pressure of H2 is (3.46 - 0.5y)

Also, from the y of reaction, mole ratio of Cl2 to HCl is 1:2, equilibrium pressure of Cl2 is (3.46 - 0.5y)

Kc = 50.1

50.1 = y^2 / (3.46 - y) (3.46 - y)

50.1 (11.9716 - 3.46y + 0.25y^2) = y^2

12.525y^2 - 173.346y + 599.77716 = y^2

11.525y^2 - 173.346y + 599.77716 = 0

y^2 - 15.04y + 52.04 = 0

The value of y is obtained using the quadratic formula

y = [15.04 - (sqrt (-15.04^2 - 4*1*52.04)) ] : 2 (1) = (15.04 - 4.25) : 2 = 10.79 : 2 = 5.40 atm (to 2 decimal places)