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Question

For the following reaction, the equilibrium constant Kc
at 298 K is 1.6×1017
Fe2+(aq)+S2(aq)FeS(s)
When equal volumes of 0.06 M Fe2+(aq) and 0.2 M S2 (aq)
solutions are mixed, the equilibrium
concentration of Fe2+(aq) is found to be Y×1017M. The value of Y is

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Solution

Fe2+(aq)+S2(aq)FeS(s) (Kc=1.6×1017
Initial 0.06 M 0.2 M
After mixing 0.03 M 0.1M
? 0.07M
1.6×1017=1[Fe2+]×0.07or[Fe2+]=10171.6×0.07=101511.2=8.928×1017 or 8.93×1017=Y×1017
or 8.93×1017=Y×1017

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