c{1}{2} \times 0.5\, M = 0.25\, M\). Similarly, for \(\mathrm{H_2}\): \(\mathrm{[H_2]}\) decreases by \(3/2 \times 0.5\, M = 0.75\, M\). Step 2: Write equilibrium concentrations: \[ \mathrm{[N_2]} = 1.0\, M - 0.25\, M = 0.75\, M \] \[ \mathrm{[
ueous solution. Solution: Molecular equation: \[ NaCl(aq) + AgNO_3(aq) \rightarrow AgCl(s) + NaNO_3(aq) \] Ionic equation: \[ Na^+(aq) + Cl^-(aq) + Ag^+(aq) + NO_3^-(aq) \rightarrow AgCl(s) + Na^+(aq) +
ogen: +1 (except metal hydrides) Sum of oxidation states in a neutral compound: 0 Sum in an ion equals its charge Example: \[ \mathrm{Fe_2O_3} \] Oxygen: -2 Total for 3 oxygens: -6 Total for 2 Fe atoms: +6 Each Fe: +3 (oxidation state) Identifying Redox Processes Oxidation
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