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Question
Balance the following reaction by oxidation number method.
\[\ce{H2SO4_{(aq)} + C_{(s)} -> CO2_{(g)} + SO2_{(g)} + H2O_{(l)}(acidic)}\]
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Solution
\[\ce{H2SO4_{(aq)} + C_{(s)} -> CO2_{(g)} + SO2_{(g)} + H2O_{(l)}(acidic)}\]
Step 1: Write the skeletal equation and balance the elements other than O and H.
\[\ce{H2SO4_{(aq)} + C_{(s)} -> CO2_{(g)} + SO2_{(g)} + H2O_{(l)}}\]
Step 2: Assign oxidation numbers to S and C. Calculate the increase and decrease in the oxidation number and make them equal.
Increase in oxidation number:
(Increase per atom = 4)
Decrease in oxidation number:
(Decrease per atom = 2)
To make the net increase and decrease equal, we must take 2 atoms of S.
\[\ce{2H2SO4_{(aq)} + C_{(s)} -> CO2_{(g)} + 2SO2_{(g)} + H2O_{(l)}}\]
Step 3: Balance ‘O’ atoms by adding H2O to the right-hand side.
\[\ce{2H2SO4_{(aq)} + C_{(s)} -> CO2_{(g)} + 2SO2_{(g)} + H2O_{(l)} + H2O_{(l)}}\]
Step 4: The medium is acidic. There is no charge on either side. Hydrogen atoms are equal on both sides.
\[\ce{2H2SO4_{(aq)} + C_{(s)} -> CO2_{(g)} + 2SO2_{(g)} + 2H2O_{(l)}}\]
Step 5: Check two sides for the balance of atoms and charges.
Hence, balanced equation is \[\ce{2H2SO4_{(aq)} + C_{(s)} -> CO2_{(g)} + 2SO2_{(g)} + 2H2O_{(l)}}\]
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