Identify the oxidizing agent and reducing agent in each of the following redox reactions.a. Al (s) + Cu^2+ (aq) → Al^3+ (aq) + Cu (s)b. Cu (s) + 2 NO3^- (aq) + 4 H^+ (aq) → Cu^2+ (aq) + 2 NO2 (g) + 2 H2O (l)
a. oxidizing agent: Cu^2+reducing agent: Al(s)b. oxidizing agent: NO3^-(aq)reducing agent: Cu(s)
a. In this redox reaction, aluminum (Al) is oxidized to form Al^3+ ions while Cu^2+ ions are reduced to form copper (Cu) atoms. Therefore, Cu^2+ ions are the oxidizing agent as they caused the oxidation of Al, while Al atoms are reducing agents because they caused the reduction of Cu^2+ ions.
b. In this redox reaction, copper (Cu) atoms are oxidized to form Cu^2+ ions while NO3^- ions are reduced to form NO2 gas and H2O molecules. Therefore, Cu atoms are the reducing agent as they caused the reduction of NO3^- ions, while NO3^- ions are the oxidizing agent as they caused the oxidation of Cu atoms. Additionally, H+ ions are present to balance the charges.
More Answers:
Identifying Anode and Cathode in a Voltaic Cell Based on Comparative Reduction PotentialsBalancing Redox Reaction in Basic Solution: Step-by-Step Guide with Examples
Balancing Redox Reaction in Acidic Solution: Step-by-Step Guide with Example
Error 403 The request cannot be completed because you have exceeded your quota. : quotaExceeded