Chemical Equations and Reactions

Chemistry B Mrs. Frost Oxidation-Reduction Homework Packet 12. Use the changes in oxidation numbers to identify which atoms are oxidized and which are reduced in each reaction. A. \[ 2 \mathrm{Na}_{(s)}+\mathrm{Cl}_{2(g)} \rightarrow 2 \mathrm{NaCl}_{(s)} \] Oxidized Reduced B. \[ 2 \mathrm{HNO}_{3(a q)}+6 \mathrm{HI}_{(a q)} \rightarrow 2 \mathrm{NO}_{(g)}+3 \mathrm{I}_{2(s)}+4 \mathrm{H}_{2} \mathrm{O}_{(\ell)} \] Oxidized Reduced C. \[ 3 \mathrm{H}_{2} \mathrm{~S}_{(g)}+2 \mathrm{HNO}_{3(a q)} \rightarrow 3 \mathrm{~S}_{(s)}+2 \mathrm{NO}_{(g)}+4 \mathrm{H}_{2} \mathrm{O}_{(\hbar)} \] Oxidized Reduced D. \[ 2 \mathrm{PbSO}_{4(s)}+2 \mathrm{H}_{2} \mathrm{O}_{(l)} \rightarrow \mathrm{Pb}_{(s)}+\mathrm{PbO}_{2(s)}+2 \mathrm{H}_{2} \mathrm{SO}_{4(a q)} \] Oxidized Reduced 13. For each reaction in Problem $\#$, identify the reducing agent and the oxidizing agent. A. \[ 2 \mathrm{Na}_{(s)}+\mathrm{Cl}_{2(g)} \rightarrow 2 \mathrm{NaCl}_{(s)} \] Oxidizing Agent Reducing Agent B. \[ 2 \mathrm{HNO}_{3(a q)}+6 \mathrm{HI}_{(a q)} \rightarrow 2 \mathrm{NO}_{(g)}+3 \mathrm{I}_{2(s)}+4 \mathrm{H}_{2} \mathrm{O}_{(l)} \] Oxidizing Agent Reducing Agent C. \[ 3 \mathrm{H}_{2} \mathrm{~S}_{(g)}+2 \mathrm{HNO}_{3(a q)} \rightarrow 3 \mathrm{~S}_{(s)}+2 \mathrm{NO}_{(g)}+4 \mathrm{H}_{2} \mathrm{O}_{(t)} \] Oxidizing Agent Reducing Agent D. \[ 2 \mathrm{PbSO}_{4(s)}+2 \mathrm{H}_{2} \mathrm{O}_{(\hbar)} \rightarrow \mathrm{Pb}_{(s)}+\mathrm{PbO}_{2(s)}+2 \mathrm{H}_{2} \mathrm{SO}_{4(a q)} \] Oxidizing Agent Reducing Agent