Problem 1
Oxidation was once defined as chemically adding oxygen to a substance. Use this reaction to argue that this definition is consistent with the modern definition of oxidation. $$ 2 \mathrm{Mg}+\mathrm{O}_{2} \rightarrow 2 \mathrm{MgO} $$
Problem 1
Define electrolytic cell.
Problem 1
Is this reaction a redox reaction? Explain your answer. $$ 2 \mathrm{~K}(\mathrm{~s})+\mathrm{Br}_{2}(\ell) \rightarrow 2 \mathrm{KBr}(\mathrm{s}) $$
Problem 1
Draw the voltaic cell represented by this reaction and label the cathode, the anode, the salt bridge, the oxidation half cell, the reduction half cell, the positive electrode, and the negative electrode. Use Figure 14.1 "A Redox Reaction in Which the Two Half Reactions Are Physically Separated" as a guide. $$ 3 \mathrm{Mg}+2 \mathrm{Cr}^{3+} \rightarrow 3 \mathrm{Mg}^{2+}+2 \mathrm{Cr} $$
Problem 1
Balance these redox reactions by inspection. a) \(\mathrm{Na}+\mathrm{F}_{2} \rightarrow \mathrm{NaF}\) b) \(\mathrm{Al}_{2} \mathrm{O}_{3}+\mathrm{H}_{2} \rightarrow \mathrm{Al}+\mathrm{H}_{2} \mathrm{O}\)
Problem 2
Is this reaction a redox reaction? Explain your answer. $$ 2 \mathrm{NaCl}(\mathrm{aq})+\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq}) \rightarrow 2 \mathrm{NaNO}_{3}(\mathrm{aq})+\mathrm{PbCl}_{2}(\mathrm{~s}) $$
Problem 2
How does the operation of an electrolytic cell differ from a voltaic cell?
Problem 2
Reduction was once defined as chemically adding hydrogen to a substance. Use this reaction to argue that this definition is consistent with the modern definition of reduction. $$ \mathrm{C}_{2} \mathrm{H}_{2}+2 \mathrm{H}_{2} \rightarrow \mathrm{C}_{2} \mathrm{H}_{6} $$
Problem 2
Balance these redox reactions by inspection. a) \(\mathrm{Fe}_{2} \mathrm{~S}_{3}+\mathrm{O}_{2} \rightarrow \mathrm{Fe}_{2} \mathrm{O}_{3}+\mathrm{S}\) b) \(\mathrm{Cu}_{2} \mathrm{O}+\mathrm{H}_{2} \rightarrow \mathrm{Cu}+\mathrm{H}_{2} \mathrm{O}\)
Problem 3
List at least three elements that are produced by electrolysis.
