Asked by Derrick
Determine the oxidation states of Se and S in the products and reactants of the following equation. Amongst the reactants, which species would be called the oxidant and which would be called the reductant?
0.5 SeO4^2- (aq) + 0.125 H2S (aq) = 0.5 SeO3^2- (aq) + 0.125 SO4^2- (aq) + 0.25 H+ (aq)
0.5 SeO4^2- (aq) + 0.125 H2S (aq) = 0.5 SeO3^2- (aq) + 0.125 SO4^2- (aq) + 0.25 H+ (aq)
Answers
Answered by
DrBob222
1. compounds must have zero charge.
2. ions must have charge on the ion.
3. oxidation states in the compound/ion must add to the charge.
For SeO4^2-, youhave
O is -2 and 4*-2 = -8 so Se must be +6 t leave a charge of -2 on the ion.
For H2S, H is +1, 2*+1 = +2 so S must be -2. The right hand side is done the same way.
The oxidizing agent (oxidant) is the one that gained electrons.
2. ions must have charge on the ion.
3. oxidation states in the compound/ion must add to the charge.
For SeO4^2-, youhave
O is -2 and 4*-2 = -8 so Se must be +6 t leave a charge of -2 on the ion.
For H2S, H is +1, 2*+1 = +2 so S must be -2. The right hand side is done the same way.
The oxidizing agent (oxidant) is the one that gained electrons.