Problem: Consider the reaction for the decomposition of hydrogen disulfide: 2H2S(g) ⇌ 2H2(g) + S2(g), Kc = 1.67 x 10–7 at 800 oC. A 0.500 L reaction vessel initially contains 0.125 mol of H2S and 0.125 mol of H2 at 800 oC. Find the equilibrium concentration of [S2].

FREE Expert Solution

[H2S] =0.215 mol0.5 L= 0.43 M

[H2] =0.215 mol0.5 L= 0.43 M



Kc = [H2]2[S2][H2S]21.67×10-7 =(0.43+2x)(x)0.43-2x(1.67×10-7)(0.43-2x) = (0.43+2x)(x)7.181×10-8 - 3.34×10-7x =0.43x + 2x2 2x2 + 0.43x - 7.181×10-8 = 0


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Problem Details

Consider the reaction for the decomposition of hydrogen disulfide: 2H2S(g) ⇌ 2H2(g) + S2(g), Kc = 1.67 x 10–7 at 800 oC. A 0.500 L reaction vessel initially contains 0.125 mol of H2S and 0.125 mol of H2 at 800 oC. Find the equilibrium concentration of [S2].

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