Question 8. Consider the following reactions: a. Zn(s) + 2 AgNO3(aq) → Zn(NO3) 2(aq) + 2 Ag(s) b. 2 Li(s) + Fe(C 2H3O 2) 2(aq) → 2 LiC2H3O 2(aq) + Fe(s) c. Ni(s) + 2 AgClO 4(aq) → Ni(ClO4) 2(aq) + 2 Ag(s) For each reaction, assign oxidation states to each element on the reactant and product side of the reaction. In addition, answer the following questions: Which element is being reduced? Which is being oxidized? What is the reducing agent? What is the oxidizing agent?
Question 8. Consider the following reactions: a. Zn(s) + 2 AgNO3(aq) → Zn(NO3) 2(aq) + 2 Ag(s) b. 2 Li(s) + Fe(C 2H3O 2) 2(aq) → 2 LiC2H3O 2(aq) + Fe(s) c. Ni(s) + 2 AgClO 4(aq) → Ni(ClO4) 2(aq) + 2 Ag(s) For each reaction, assign oxidation states to each element on the reactant and product side of the reaction. In addition, answer the following questions: Which element is being reduced? Which is being oxidized? What is the reducing agent? What is the oxidizing agent?
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter3: Chemical Reactions
Section3.5: Oxidatino-reduction And Electron Transfer
Problem 3.12CE
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Question 8.
Consider the following reactions:
a. Zn(s) + 2 AgNO3(aq) → Zn(NO3) 2(aq) + 2 Ag(s)
b. 2 Li(s) + Fe(C 2H3O 2) 2(aq) → 2 LiC2H3O 2(aq) + Fe(s)
c. Ni(s) + 2 AgClO 4(aq) → Ni(ClO4) 2(aq) + 2 Ag(s)
For each reaction, assign oxidation states to each element on the reactant and product side of the
reaction. In addition, answer the following questions: Which element is being reduced? Which is being
oxidized? What is the reducing agent? What is the oxidizing agent?
Question 9.
Write and balance the complete ionic and net ionic equations for each acid base reaction:
a. HI (aq) + RbOH(aq) → H2O (l) + RbI (aq)
b. NaOH + HNO 3 (aq) → H2O (l) + NaNO 3 (aq)
c. HCl (aq) + LiOH (aq) → LiCl (aq) + H2O (l
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