A sealed 1.0 L flask is charged with 0.500 mol of I₂ and 0.500 mol of Br₂. An equilibrium reaction ensues: I₂ (g) + Br₂ (g) 2IBr (g)
When the container contents achieve equilibrium, the flask contains 0.84 mol of IBr. The value of K_eq is ________.

Question

A sealed 1.0 L flask is charged with 0.500 mol of I₂ and 0.500 mol of Br₂. An equilibrium reaction ensues: I₂ (g) + Br₂ (g)

A sealed 1.0 L flask is charged with 0.500 mol of I<sub>2</sub> and 0.500 mol of Br<sub>2</sub>. An equilibrium reaction ensues: I<sub>2</sub> (g) + Br<sub>2</sub> (g) 2IBr (g) When the container contents achieve equilibrium, the flask contains 0.84 mol of IBr. The value of K<sub>eq</sub> is ________. A) 11 B) 4.0 C) 110 D) 6.1 E) 2.8

2IBr (g)
When the container contents achieve equilibrium, the flask contains 0.84 mol of IBr. The value of K_eq is ________.

Quizplus · Accepted Answer

We can set up an ICE table to help us solve for the equilibrium constant, K: I₂(g) + Br₂(g) 11ea7cce_1f6a_c6b9_a2ab_8587c197a806_TB2701_11 2IBr(g) I 0.500 mol 0.500 mol -0.84 mol B 0.500 mol 0.500 mol -0.84 mol C 0.500-0.84 mol 0.500-0.84 mol 0.84 mol E ? ? ? Using the values in the table, we can plug them into the equilibrium expression and solve for K: K = [IBr]^2/([I₂]*[Br₂]) K = (0.84 mol)^2/((0.500-0.84 mol)*(0.500-0.84 mol)) K = 110 Therefore, the value of K is 110, and the correct answer is choice (C).

A Sealed 1