a) Balance the reaction. Find oxidant and reducer: H_(2)O_(2)+KMnO_(4)-H_(2)SO_(4)arrow O_(2)+MnSO_(4)+K_(2)SO_(4)+H_(2)O

To balance the reaction, we need to ensure that the number of atoms of each element is the same on both sides of the equation. Let's start by balancing the oxygen atoms:<br /><br />$H_{2}O_{2} + KMnO_{4} + H_{2}SO_{4} \rightarrow O_{2} + MnSO_{4} + K_{2}SO_{4} + H_{2}O$<br /><br />Next, we balance the hydrogen atoms:<br /><br />$H_{2}O_{2} + KMnO_{4} + H_{2}SO_{4} \rightarrow O_{2} + MnSO_{4} + K_{2}SO_{4} + 2H_{2}O$<br /><br />Now, we balance the potassium atoms:<br /><br />$H_{2}O_{2} + 2KMnO_{4} + H_{2}SO_{4} \rightarrow O_{2} + 2MnSO_{4} + K_{2}SO_{4} + 2H_{2}O$<br /><br />Finally, we balance the manganese atoms:<br /><br />$H_{2}O_{2} + 2KMnO_{4} + 3H_{2}SO_{4} \rightarrow O_{2} + 2MnSO_{4} + K_{2}SO_{4} + 2H_{2}O$<br /><br />Now, let's identify the oxidizing and reducing agents:<br /><br />Oxidizing agent: KMnO4 (Potassium permanganate) - It gains electrons and is reduced to MnSO4.<br /><br />Reducing agent: H2O2 (Hydrogen peroxide) - It loses electrons and is oxidized to O2.