A sealed 1.0 L flask is charged with 0.500 mol of I2 and 0.500 mol of...

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) ↔ 2 IBr(g).

When the reaction reaches equilibrium, the flask contains 0.640 mol of IBr. What is the value of the equilibrium constant K_c, for this reaction?

Expert Solution

I₂(g) + Br₂(g) ↔ 2 IBr(g).

I 0.5 0.5 0

C 0.32 0.32 0.64

E 0.18 0.18 0.64

Kc = [IBr]²/[I2][Br2]

= (0.64)²/0.18*0.18 = 12.64

queen_honey_blossom answered 2 years ago

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