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The reaction 2H2S(g)⇌2H2(g)+S2(g) Kc=1.67×10−7 at 800∘C is carried out with the following initial concentrations: [H2S] =...

The reaction 2H2S(g)⇌2H2(g)+S2(g) Kc=1.67×10−7 at 800∘C is carried out with the following initial concentrations: [H2S] = 0.150 M , [H2] =0.375 M , and [S2] = 0.00 M. Find the equilibrium concentration of  [S2].

Solutions

Expert Solution

2H2S(g) <--------------------> 2H2(g)   +   S2(g)

0.150                                    0.375    0     ------------------------> initial

0.150-2x                                 0.375 +2x     x -------------------> equilibrium

Kc = [H2]^2 [S2]/[H2S]^2

Kc = (0.375 +2x)^2   (x) / (0.150-2x   )^2

1.67 x 10^-7 = (0.375 +2x)^2   (x) / (0.150-2x   )^2

4x^3 - 6.68 x 10^-7 x^2 + 0.141x -9.64 x 10^-8 = 0

by solving this equation

x = 6.84 x 10^-7

[S2] = x = 6.84 x 10^-7 M

equilibrium concentration = 6.84 x 10^-7 M

queen_honey_blossom answered 1 year ago
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