System: Prediction: Should you expect H₂(g) to be evolved? Why or why not? What gas(es) might be emitted if the nitrate ion reacts? Observations: Net ionic equation for the reaction, if any #1: Cu and HNO3 System 3: NaHSO3 and KMnO4 Prediction Is the HSO; ion a possible oxidizing agent? If yes, to what species could it change? Is it a possible reducing agent? If yes, to what species could it change? # 2: Cu and HCI Is the MnO4 ion a possible oxidizing agent? If yes, list the species to which it could change, their colors and conditions that favor each change: Why is the MnO4 ion not a possible reducing agent?

Since you have asked multiple questions, we will answer the first one for you To get the remaining question solved, please repost the complete question which you want us to solve.1) In the reaction involving copper and nitric acid as reactants, H2 gas is not evolved. This is because nitric acid is a strong oxidizing agent which oxidizes H2 to H2O and itself gets reduced to nitrogen oxides. When the nitrate ion reacts, redox reaction takes place in which copper is oxidized to Cu2+ forming copper nitrate, hydrogen oxidized to water and nitrate ion itself reduces to any of the nitrogen oxide gases- N2O, NO, NO2. For example: Cu (s)+4HNO3 (aq)→Cu(NO3)2 (aq) +2NO2 (g)+2H2O (l) Observation- the solution turns blue as a result of oxidation of Cu to Cu2+. Net ionic equation: Cu (s)+4H++4NO3- (aq)→Cu2+(aq)+2NO3- (aq) +2NO2 (g)+2H2O (l)≡Cu (s)+4H++2NO3- (aq)→Cu2+(aq)+2NO2 (g)+2H2O (l)2) No reaction takes place between copper and hydrochloric acid since copper is below hydrogen in the activity series and thus, copper will not displace hydrogen from hydrochloric acid and thus, hydrogen gas is not evolved. Observation- No change observed. Net ionic equation: Cu(s)+HCl(aq)→No Reaction