Chemical Reactions
Recognizing reduction and oxidation
For each chemical reaction listed in the table below, decide whether the highlighted atom is being oxidized or reduced.
\begin{tabular}{|c|c|c|c|}
\hline \multirow[b]{2}{*}{reaction} & \multicolumn{3}{|l|}{highlighted atom is being...} \\
\hline & oxidized & reduced & neither oxidized nor reduced \\
\hline \( 2 \mathrm{NH}_{3}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq}) \rightarrow\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}(a q) \) & \( \bigcirc \) & \( \bigcirc \) & - 0 \\
\hline \( \mathrm{CH}_{4}(\mathrm{~g})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \rightarrow 4 \mathrm{H}_{2}(\mathrm{~g})+\mathrm{CO}_{2}(g) \) & \( \bigcirc \) & \( \bigcirc \) & \( \bigcirc \) \\
\hline \( \mathrm{CO}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \rightarrow \mathrm{CO}_{2}(\mathrm{~g})+\mathrm{H}_{2}(\mathrm{~g}) \) & \( \bigcirc \) & 0 & 0 \\
\hline \( 2 \mathrm{Cl}^{-}(\mathrm{aq})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \rightarrow 2 \mathrm{OH}^{-}(\mathrm{aq})+\mathrm{H}_{2}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g}) \) & O. & 0 & 0 \\
\hline
\end{tabular}
Explanition
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