Consider the reaction for the decomposition of hydrogen disulfide: 2H2S(g)⇌2H2(g)+S2(g), Kc = 1.67×10−7 at 800∘C A...

Consider the reaction for the decomposition of hydrogen disulfide: 2H2S(g)⇌2H2(g)+S2(g),

Kc = 1.67×10−7 at 800∘C
A 0.500 L reaction vessel initially contains 5.00×10⁻² mol of H2S and 8.75×10⁻² mol of H2 at 800∘C.

Find the equilibrium concentration of [S2].

Expert Solution

queen_honey_blossom answered 2 years ago

Consider the reaction for the decomposition of hydrogen disulfide: 2H2S(g)⇌2H2(g)+S2(g), Kc=1.67×10−7 at 800∘C The reaction is carried...

Consider the reaction for the decomposition of hydrogen disulfide: 2H2S(g)⇌2H2(g)+S2(g), Kc=1.67×10−7 at 800∘C The reaction is carried out at the same temperature with the following initial concentrations: [H2S][H2][S2]===4.50×10−4M0.00M0.00M Find the equilibrium concentration of S2.

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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] = 0.150 M , [H2] =0.375 M , and [S2] = 0.00 M. Find the equilibrium concentration of [S2].

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