1)If the reactant is MnO4- and the product is MnO42-, calculate the change in th
ID: 1001480 • Letter: 1
Question
1)If the reactant is MnO4- and the product is MnO42-, calculate the change in the oxidation state of manganese (oxidation state of manganese in product minus the oxidation state of manganese in the reactant). Enter the sign and magnitude of the result, and separated by a comma, also enter O or R to indicate whether manganese is oxidized (O) or reduced (R). Example: -2,O.
2)In a half reaction where the product is H+ and the reactant is H-, the chemical process is called________ and the number of electrons involved is _______.
3)If the product is Mn2+ and the reactant is Mn, then Mn is called a______ agent and the number of electrons transferred is______ .
4)If the product is Rb+ and the reactant is Rb, then Rb is called a _____ agent and the number of electrons transferred is ______ .
5)If the product is H2SO3 and the reactant is S, then S is called a______ agent and the number of electrons transferred is_____ .
6)If the product is ClO2- and the reactant is ClO3-, then ClO3- is called a _____ agent and the number of electrons transferred is ________ .
Explanation / Answer
1. The required reaction is MnO4- + e = MnO4-2 and the oxidation no of Mn in the reactant is +7 and in the product that is +6 so Mn is reduced so the ans is -1, R
2. The chemical process is oxidation and 2 electrons are involved here.
3. As the oxidation of Mn is taking place so it acts as a reducing agent and the no of electrons transferred is 2.
4. As the oxidation of Rb is taking place so it acts as a reducing agent and the no of electrons tranferred is 1.
5. The required reaction is S+ 3H2O = H2SO3 +4H+ +4e so S acts as a reducing agent and 4 electrons are involved.
6. The required reaction is ClO3-+ 2H+ + e = ClO2- + H2O so ClO3- acts as an oxidising agent and only 1 electron is involved.
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