Pad 3:59 PM * 60% ?session.masteringchemistry.com ¢ MasteringChemistry: Chapter

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Pad 3:59 PM * 60% ?session.masteringchemistry.com ¢ MasteringChemistry: Chapter 15 Exercise 15.82 MasteringChemistry Kwik Learning Online (4) Jungle Deals Blog 17 of 24 Consider the following reaction: 2H2S(g) +SO2(g)3S(s) +2H20(9) A reaction mixture initially containing 0.520 M H2S and 0.520 M S02 was found to contain 1.3x03 M H20 at a certain temperature. A second reaction mixture at the same temperature initially contains H2S 0.260 M and SO20.335 M Part A Calculate the equilibrium concentration of H2O in the second mixture at this temperature Express your answer using two significant figures. H20] Request Answer Next

Explanation / Answer

Equilibrium constant expression for the reaction

K = [H2O]2 / [SO2] [H2S]2

K = [1.3*10^-3]2 / [0.520] [0.520]2

K = 0.00000169 / (0.140608)

K = 1.20*10^-5

For second reaction mixture K is constant

K = [H2O]2 / [SO2] [H2S]2

1.20*10^-5 =  [H2O]2 / [0.335] [0.260]2

[H2O]2 = 1.20*10^-5 x 0.022646 = 2.72 x 10^-7

[H2O] = 5.21*10^-4 M

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