We have... Cu(s) + AgNO_3(aq) => Cu(NO_3)_2(aq) + Ag(s) A. What is the oxidation

Question

We have... Cu(s) + AgNO_3(aq) => Cu(NO_3)_2(aq) + Ag(s) A. What is the oxidation state of every atom on the reactant side? B. What is the oxidation state of every atom on the product side? C. Which atom experienced an increase in oxidation number? This atom has been oxidized during the course of this action. D. Was an electron lost or gained by this atom in the reaction? E. How many electrons were lost by this atom? F. Which atom experienced a decrease in oxidation number? G. Was an electron lost or gained by this atom in the reaction? H. How many electrons were gained by this atom?

Explanation / Answer

follow this redox. Cu is oxidized from 0 in Cu(s) to +2 in Cu(NO3)2(aq). Ag is reduced from +1 in AgNO3(aq) to 0 in Ag(s). In a double displacement or precipitaion reaction, there should not be a change in oxidation state. In an acid base reaction, there should exist water or a salt being formed.

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