What would be the equivalent weight of reductant inthe given reaction?36 2 2[Fe(CN) ] H O 2OH− −+ + →46 2 22[Fe(CN) ] 2H O O− +

To determine the equivalent weight of the reductant in the given reaction, we need to follow these steps:

Step 1: Identify the reductant in the reaction. In this case, the reductant is [Fe(CN)6]4-.

Step 2: Determine the change in oxidation state of the reductant. In the reaction, [Fe(CN)6]4- is being reduced from a +2 oxidation state to a +4 oxidation state.

Step 3: Calculate the change in the number of electrons transferred during the reaction. Since the oxidation state of [Fe(CN)6]4- increases by 2, it means that 2 electrons are being transferred.

Step 4: Determine the molar mass of the reductant. The molar mass of [Fe(CN)6]4- can be calculated by adding the atomic masses of each element in the compound: Fe (55.85 g/mol) + C (12.01 g/mol) + N (14.01 g/mol) + 6 * C (12.01 g/mol) = 211.09 g/mol.

Step 5: Calculate the equivalent weight of the reductant. The equivalent weight is calculated by dividing the molar mass of the reductant by the number of electrons transferred. In this case, the equivalent weight would be 211.09 g/mol / 2 electrons = 105.55 g/equivalent.

Therefore, the equivalent weight of the reductant in the given reaction is 105.55 g/equivalent.