10. The equilibrium constant Kc for the
reaction
H2(g) + Br2(g) ⇆ 2HBr(g) |
is 2.180 × 106 at 730°C. Starting with 2.20 moles of HBr
in a 13.7−L reaction vessel, calculate the concentrations of
H2, Br2, and HBr at equilibrium.
[H2] | = | |
[Br2] | = | |
[HBr] | = |
The reaction is as shown below
The equilibrium constant
Calculate initial concentration of HBr
Let 2x M be the change in the concentration of HBr to reach equilibrium. Prepare an ICE table.
Initial concentration (M) | 0.00 | 0.00 | 0.161 |
Change in concentration (M) | x | x | -2x |
Equilibrium concentration (M) | x | x |
Substitute values in the equilibrium constant expression
Since the value of the equilibrium constant is very large, approximate 0.161-2x to 0.161
Take square root on both sides
Hence, the equilibrium concentrations are calculated as shown below
10. The equilibrium constant Kc for the reaction H2(g) + Br2(g) ⇆ 2HBr(g) is 2.180 ×...
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