Using the following data,determine for the electrochemical cell constructed using the reaction of nitrous oxide and oxalic acid under acidic conditions.Unbalanced: N₂O(g)+ H₂C₂O₄(s)$\to$ 2 CO₂(g)+ N₂(g)+ H₂O( ) Half-reaction Standard reduction potential 2 CO₂(g)+ 2 H⁺(aq)+ 2 e^- $\to$ H₂C₂O₄(s)-0.49 N₂O(g)+ 2 H⁺(aq)+ 2 e^-$\to$ N₂(g)+ H₂O( )+1.78

Question

Quizplus · Accepted Answer

The standard potential of the half-reaction for the reduction of nitrous oxide to nitric oxide is +1.78 V, and the standard potential of the half-reaction for the reduction of oxalic acid to carbon dioxide is +0.49 V. To determine the overall cell potential, we need to subtract the reduction potential of the anode half-reaction from the reduction potential of the cathode half-reaction. This gives:

+0.49 V - (+1.78 V) = +2.27 V

Therefore, the answer is choice C, "+2.27 V".

Using the Following Data,determine for the Electrochemical Cell Constructed →\to→

Using the Following Data,determine for the Electrochemical Cell Constructed $\to$