1. Balance the redox equation: K_(1)Fe(CN)_(6)+H_(2)SO_(4)+H_(2)O=K_(2)SO_(4)+FeSO_(4)+(NH_(3))_(2)SO_(4)+CO_(4)

To balance the redox equation, we need to follow these steps:1. Identify the oxidation states of each element in the equation.2. Determine which elements are being oxidized and reduced.3. Balance the atoms of the elements that are being oxidized and reduced.4. Balance the charge by adding electrons to the appropriate side of the equation.5. Balance the remaining atoms in the equation.Let's start by identifying the oxidation states of each element in the equation: In this equation, the oxidation states are as follows:K: +1Fe: +2C: +4N: -3H: +1S: +6O: -2Now, let's determine which elements are being oxidized and reduced:Fe is being reduced from an oxidation state of +2 to +2 in FeSO4.C is being oxidized from an oxidation state of +4 in K1Fe(CN)6 to +4 in CO4.Next, we balance the atoms of the elements that are being oxidized and reduced:Fe: 1 atom on both sidesC: 6 atoms on the left side and 1 atom on the right sideTo balance the charge, we add electrons to the appropriate side of the equation: Finally, we balance the remaining atoms in the equation:K: 2 atoms on the right sideH: 8 atoms on the left side and 8 atoms on the right sideS: 1 atom on the left side and 1 atom on the right sideO: 12 atoms on the left side and 12 atoms on the right sideThe balanced redox equation is: