Question- 1. Balance the following redox reaction (make sure to write BOTH the balanced oxidation and reduction half-reactions). Indicate those elements that undergo changes in oxidation number, and specify the oxidation state before and after reaction.
H2C2O4(aq)+NO3^-(aq)--> CO2(g)+NO(g)
2. A voltaic cell utilizes the following reaction:
MnO4^-(aq)+Cr(OH)3(s)+OH^-(aq)-->MnO2(s)+CrO4^2-(aq)+2H2O(l)
What is the potential of this cell under standard conditions Ecell? Is this reaction spontaneous under standard conditions at 25degreesC?
3. If the concentrations of MnO4^- and CrO4^2- are both .1M, at what pH would the potential of this cell be .60V at 25degrees C?
Please take care to answer each question mark in the equations