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Current Question (ID: 8575)
Question:
$\text{The balanced equation for the reaction between chlorine and sulphur dioxide in water is:}$
Options:
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1. \text{Cl}_2\text{(s)} + \text{SO}_2\text{(aq)} + 2\text{H}_2\text{O(l)} \rightarrow 2\text{Cl}^-\text{(aq)} + \text{SO}_4^{2-}\text{(aq)} + 4\text{H}^+\text{(aq)}
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2. 3\text{Cl}_2\text{(s)} + \text{SO}_2\text{(aq)} + 2\text{H}_2\text{O(l)} \rightarrow \text{Cl}^-\text{(aq)} + \text{SO}_4^{2-}\text{(aq)} + 3\text{H}^+\text{(aq)}
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3. \text{Cl}_2\text{(s)} + 3\text{SO}_2\text{(aq)} + \text{H}_2\text{O(l)} \rightarrow \text{Cl}^-\text{(aq)} + 2\text{SO}_4^{2-}\text{(aq)} + 4\text{H}^+\text{(aq)}
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4. 2\text{Cl}_2\text{(s)} + \text{SO}_2\text{(aq)} + \text{H}_2\text{O(l)} \rightarrow 2\text{Cl}^-\text{(aq)} + \text{SO}_4^{2-}\text{(aq)} + 4\text{H}^+\text{(aq)}
Solution:
\text{Hint: Total charge should be balanced in the reaction.}
\text{Explanation:}
\text{The given redox reaction can be represented as:}
\mathrm{Cl_2(s) + SO_2(aq) + H_2O(l) \rightarrow Cl^-(aq) + SO_4^{2-}(aq)}
\text{The oxidation half reaction is:}
\mathrm{S^{+4}O_2(aq) \rightarrow S^{+6}O_4^{2-}(aq)}
\text{The oxidation number is balanced by adding two electrons as:}
\mathrm{SO_2(aq) \rightarrow SO_4^{2-}(aq) + 2e^-}
\text{The charge is balanced by adding 4H}^+ \text{ ions as:}
\mathrm{SO_2(aq) \rightarrow SO_4^{2-}(aq) + 4H^+(aq) + 2e^-}
\text{The O atoms and H}^+ \text{ ions are balanced by adding 2H}_2\text{O molecules as:}
\mathrm{SO_2(aq) + 2H_2O(l) \rightarrow SO_4^{2-}(aq) + 4H^+(aq) + 2e^-} \quad \text{....(i)}
\text{The reduction half reaction is:}
\mathrm{Cl_2(s) \rightarrow Cl^-(aq)}
\text{The chlorine atoms are balanced as:}
\mathrm{Cl_2^0(s) \rightarrow 2Cl^{-1}(aq)}
\text{The oxidation number is balanced by adding electrons:}
\mathrm{Cl_2(s) + 2e^- \rightarrow 2Cl^-(aq)} \quad \text{......(ii)}
\text{The balanced chemical equation can be obtained by adding equation (i) and (ii) as:}
\mathrm{Cl_2(s) + SO_2(aq) + 2H_2O(l) \rightarrow 2Cl^-(aq) + SO_4^{2-}(aq) + 4H^+(aq)}
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