91影视

1. Write the unbalanced half-reaction: NO鈧冣伝 鈫� NO 2. Balance the atoms other than oxygen and hydrogen: In this case, the nitrogen atoms are already balanced. 3. Balance the oxygen atoms by adding water molecules: Since there are 3 oxygen atoms in the reactant and only 1 in the product, we need to add 2 water molecules to the product side: NO鈧冣伝 鈫� NO + 2H鈧侽 4. Balance hydrogen atoms by adding H鈦� ions: Since we have 4 hydrogen atoms on the product side, we need to add 4 H鈦� ions to the reactant side: NO鈧冣伝 + 4H鈦� 鈫� NO + 2H鈧侽 5. Balance the charges by adding electrons: The overall charge on the reactant side is 1鈦� + 4鈦� = 3鈦�, while the overall charge on the product side is 0. Therefore, we need to add 3 electrons to the reactant side to balance the charges: NO鈧冣伝 + 4H鈦� + 3e鈦� 鈫� NO + 2H鈧侽 Finally, the balanced half-reaction for the reduction of nitrate ion to NO in acidic solution is: \(NO_3^- + 4H^+ + 3e^- 鈫� NO + 2H_2O\).

1. Write the unbalanced half-reaction: HNO鈧� 鈫� NO鈧� 2. Balance the atoms other than oxygen and hydrogen: In this case, the nitrogen atoms are already balanced. 3. Balance the oxygen atoms by adding water molecules: There are 2 oxygen atoms on both the reactant and the product, so no water molecules need to be added. 4. Balance hydrogen atoms by adding H鈦� ions: Since we have 1 hydrogen atom in the reactant and none in the product, we need to add 1 H鈦� ion to the product side: HNO鈧� 鈫� NO鈧� + H鈦� 5. Balance the charges by adding electrons: The overall charge on the reactant side is 0, while the overall charge on the product side is 1鈦�. Therefore, we need to add 1 electron to the product side to balance the charges: HNO鈧� 鈫� NO鈧� + H鈦� + e鈦� Finally, the balanced half-reaction for the oxidation of HNO鈧� to NO鈧� in acidic solution is: \(HNO_2 鈫� NO_2 + H^+ + e^-\).