The following equilibrium was studied by analyzing the equilibrium mixture for t

Question

The following equilibrium was studied by analyzing the equilibrium mixture for the amount of H2S produced.

Sb2S3(s)+H2(g)--->Sb(s)+H2S(g) (unbalanced). A vessel whose volume was 2.50L was filled with 0.0100 mol antimony(III) sulfide and 0.0100 mol hydrogen. After the mixture came to equilibrium in the closed vessel at 440 C, the gaseous mixture was removed and the hydrogen sulfide was dissolved in water. Sufficient lead (II) ion was added to react completely with the hydrogen sulfide to precipitate 1.029g PbS. What is the value of a)K and b)deltaG?

Explanation / Answer

a) K=[H2S]3/[H2]3=(0.0043)3/(0.0057)3=0.429

b) deltaG=-RTlnK=-8.314*713K*ln0.429=5012.3 J/m*K

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