Problem: Consider the following reaction: NH4HS(s) ⇌ NH3(g) + H2S(g)At a certain temperature, Kc = 8.5 x 10–3. A reaction mixture at this temperature containing solid NH4HS has [NH3] = 0.166 and [H2S] = 0.166. Will more of the solid form or will some of the existing solid decompose as equilibrium is reached?

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Q = productreactantQ=[NH3][H2S]Q = (0.166)(0.166)

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Problem Details

Consider the following reaction: NH4HS(s) ⇌ NH3(g) + H2S(g)

At a certain temperature, Kc = 8.5 x 10–3. A reaction mixture at this temperature containing solid NH4HS has [NH3] = 0.166 and [H2S] = 0.166. Will more of the solid form or will some of the existing solid decompose as equilibrium is reached?

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Based on our data, we think this problem is relevant for Professor Delgado's class at FIU.