Question: For each of the following redox reactions, a) Write out the balanced net ionic equation. b) Write the anode (oxidation) half-reaction. c) Write the

For each of the following redox reactions, a) Write out the balanced net ionic equation. b) Write the anode (oxidation) half-reaction. c) Write the cathode (reduction) half-reaction. d) Identify both the oxidizing agent and the reducing agent. e) Look up each half-reaction potential and calculate the standard cell potential (E). f) Is the reaction spontaneous at standard conditions? 1. 3Cu(s) + 8HNO3(aq) 3Cu(NO3)2(aq) + 2NO(g) + 4HO(4) 42 2. Zn(s) + 2HCl(aq) ZnCl(aq) + H(g) -

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a 3Cus 8HNO3aq 3CuNO32aq 2NOg 4H2Ol Net ionic equation 3Cus 4Haq 8NO3aq 3Cu2aq 2NOg 4H2Ol b Anode ox... View full answer

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