If the reactant is IO3- and the product is IO4-, calculate the change in the oxi
ID: 1001474 • Letter: I
Question
If the reactant is IO3- and the product is IO4-, calculate the change in the oxidation state of iodine (oxidation state of iodine in product minus the oxidation state of iodine in the reactant). Enter the sign and magnitude of the result, and separated by a comma, also enter O or R to indicate whether iodine is oxidized (O) or reduced (R). Example: -2,O.
If the reactant is Br2 and the product is BrO-, then Br2 is called a ______ agent and the number of electrons transferred is _______ .
If the product is CO and the reactant is CO2, then CO2 is called a ______ agent and the number of electrons transferred is _______.
If the reactant is HNO2 and the product is NO, calculate the change in the oxidation state of nitrogen (oxidation state of nitrogen in product minus the oxidation state of nitrogen in the reactant). Enter the sign and magnitude of the result, and separated by a comma, also enter the number of electrons gained or lost (no signs) by an atom of nitrogen. Example: -2,2.
If the reactant is Sn2+ and the product is Sn4+, calculate the change in the oxidation state of tin (oxidation state of tin in product minus the oxidation state of tin in the reactant). Enter the sign and magnitude of the result, and separated by a comma, also enter O or R to indicate whether tin is oxidized (O) or reduced (R). Example: -2,O.
If the reactant is S2O82- and the product is SO42-, calculate the change in the oxidation state of sulfur (oxidation state of sulfur in product minus the oxidation state of sulfur in the reactant). Enter the sign and magnitude of the result, and separated by a comma, also enter the number of electrons gained or lost (no signs) by an atom of sulfur. Example: -2,2.
Explanation / Answer
(A) The oxidation state of iodine in IO3- is +5 and the oxidation state of iodine in IO4- is +7
Change in oxidation state of iodine = (+7 - +5) = +2
The process is oxidation.
Answer: +2, O
(B) Oxidation state of bromine in Br2 is 0 and in BrO- is +1
Bromine undergoes oxidation.
Therefore, Br2 is called a reducing agent and the number of electrons transferred = ( +1 -0 ) = 1
(C) The oxidation state of carbon in CO is +2 and the oxidation state of carbon in CO2 is +4.
Therefore, carbon in CO2 undergoes reduction to form CO.
Thus, CO2 is called an oxidizing agent and the number of electrons transferred is ( +4 - +2) = 2
(D) Oxidation state of nitrogen in HNO2 is +3 and in NO the oxidation state is +2
Therefore, nitrogen in HNO2 undergoes reduction to form NO.
Change in oxidation state = (+3 - +2) = + 1
Answer: +1, 1
(E) Change in oxidation state of tin = (+4 - +2) = +2
Tin in Sn2+ undergoes oxidation to form Sn+4
Answer: +2, O
(F) Oxidation state of sulfur in S2O8-2 is +7 and in SO4-2it is +6
Change in oxidation state of sulfur = +2
Answer: +2, 2