In the following unbalanced redox reaction: Fe^+2 (aq) + O_2 (g) rightarrow Fe^+

Question

In the following unbalanced redox reaction: Fe^+2 (aq) + O_2 (g) rightarrow Fe^+3 _aq) H_2 O_(l) Will this reaction be spontaneous in 0.100 M HCI if the iron (II) and iron (III) concentrations are 0.100 M and 0.200 M respectively. Assume the molarity of oxygen gas is 1. The reaction will be spontaneous and strongly favor the products The reaction will be spontaneous but only slightly favor the products The reaction will be nonspontaneous but only slightly favor the reactants The reaction will be nonspontaneous but strongly favor the reactants None of the above

Explanation / Answer

4Fe+2(aq) + O2(g) + 4H+(aq) -------------> 4Fe+3(aq) + 2H2O

is the balanced equation.

SRP of Fe+3/FE+2 = +0.79 V

O2/ h2O = +1.23V

Thus the Ecell of theis reaction is =1.23-0.79 = 0.44V

As the Ecell is positive the reaction is spontaneou s and strongly favors the products.

Option A

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