The equilibrum constant Kc is 0.01323 for the reaction: CCl4 (g) <----> C(s) + 2 Cl2...

The equilibrum constant Kc is 0.01323 for the reaction: CCl4 (g) <----> C(s) + 2 Cl2 (g)

At 300k a 5L flask originally contained 0.0828M of CCl4, 0.0444 M of C and 0.0546M of Cl2. Determine the concentration of Cl2 when equilibrium is reached.

Solutions

Expert Solution

CCl4 (g) <----> C(s) + 2 Cl2 (g)

I 0.0828 0.0444 0.0546

C +x -x -x

E 0.0828+x 0.0444-x 0.0546-x

Kc = [Cl2]^2/[CCl4]

0.01323 = (0.0546-x)^2/0.0828+x

0.01323(0.0828+x) = (0.0546-x)^2

x = 0.018

[Cl2] = 0.0546-x = 0.0546-0.018 = 0.0366M >>>>>answer

queen_honey_blossom answered 1 year ago

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