Net Potential for Reaction Products: Fe2+ + Co3+ & CrO42- + MoO2

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The discussion focuses on determining the net potential for two chemical reactions involving Fe2+ and Co3+, as well as CrO42− and MoO2, under acidic conditions. For the first reaction, it is concluded that no reaction occurs because Co3+ is not a strong enough oxidizer to oxidize Fe2+. In the second reaction, the balanced equation is provided, showing the conversion of CrO42− and MoO2 into Cr2O72− and water, with Mo being oxidized to Mo4+. The rationale behind these conclusions is based on trends in oxidation states. Overall, the analysis emphasizes the importance of understanding oxidation potentials in predicting reaction outcomes.
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Homework Statement



For each reaction, give balanced chemical equations or NR (no reaction) and rationalize your answers in terms of trends in oxidation states. Calculate net potential for the reactions:

a) Fe2+(aq) + Co3+ (aq) (acidic conditions) →b) CrO42−(aq) + MoO2(s) + H+ (acidic conditions) →

Homework Equations


The Attempt at a Solution



a) no reaction

b) 2CrO42−(aq) + MoO2(s) + 4H+ → Cr2O72- + 2H2O + Mo4+

Is this correct?
 
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In the first case you are asked whether Co3+ is an oxidizer strong enough to oxidize Fe2+. Second question is similar.
 
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