Fe2O3(s) may be converted to Fe by the reaction Fe2O3(s)+3H2(g)⇌2Fe(s)+3H2O(g) for which Kc = 8 at temp. 720oC What percentage of the H2 remains unreacted after the reaction has come to equilibrium?

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≃22%

≃34%

≃66%

=78%

answer is B.

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Detailed Solution

Let initial moles of H2(g) is 1 Fe2O3(s)+3H2(g)⇌2Fe(s)+3H2O(g) at eq.; 1-3x 3x Kc=3xV31-3xV3 ⇒ 8=3x1-3x3 x =0.22 % of H2 unreacted =1-3×0.221×100=34

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