KMnO4+NaCl+H2SO4----->Cl2+K2SO4+MnSO4+H2O+Na2SO4 identify the atom oxidized, the atom reduced, balance the equation and write the net ionic equation

Complete and balance the following redox reaction in basic solution MnO,-(aq) + C,0,²-(aq) → MnO,(s) + CO2(g)

In the above redox reaction, use oxidation numbers to identify the element oxidized, the element reduced, the oxidizing agent and the reducing agent. name of the element oxidized: 3Ag + Cr³+→→→→Cr + 3Ag+ formula of the oxidizing agent: name of the element reduced: formula of the reducing agent:

Identify whether each of the following reaction is a redox reaction. If it is so, by showing the change in oxidation numbers identify the oxidizing agent and reducing agent. 4 CaSO3 ⟶ 3 CaSO4 + CaS 2 KMnO4+ 3 H2O2 → 2 MnO2 + 2 KOH + 2 H2O + 3 O2

After balancing the following redox equation, the sum of the stoichiometric coefficients on the right-hand side of the equation is: Cu²+ (aq) + Ce³+ (aq) + H₂O(1) → CeO₂(s) + Cu(s) + H+ (aq) [not balanced] 02 O 3 Q7 O 9 00 11

Write your answer in the blank provided. Examine the following balanced half-reaction:  2H2O + CrO2 → CrO4 2- + 3e- + 4H+  1. Is this an oxidation or a reduction? 2. What element is oxidized or reduced?      Balance the following half-equation in acid. ClO3 - → Cl2 The above reaction occurs along with the reaction given above before Part 1 of this problem.  Write a balanced equation for the overall reaction that occurs.  What is the coefficient of water in the balanced overall equation? Which reactant is the oxidizing agent?

For the following redox reaction, write a balanced equation for the whole reaction and include the states of matter: MnO4 (aq) + Cl (aq) → Mn²+ (aq) + Cl₂(g) (in acidic solution) Balanced equation: ->>>

2Cl- + SS2- + Cl2 In the above redox reaction, use oxidation numbers to identify the element oxidized, the element reduced, the oxidizing agent and the reducing agent.