The reaction
SO₂Cl₂ → SO₂ + Cl₂is a first order reaction with k = 2.2 x 10^–5s^–1 at 320° C. Calculate the percentage of SO₂Cl₂ that is decomposed on heating this gas for 30 minutes.

Solution

The reaction
SO₂Cl₂ → SO₂ + Cl₂is a first order reaction with k = 2.2 x 10^–5s^–1 at 320° C
Thus by using the first order equation

k = \frac{2.303}{t} \log \frac{[A_{0}]}{[A]}

\Rightarrow = \log \frac{100}{[A]} = \frac{2.2 \times 10^{- 5} \times 30 \times 60}{2.303}

\log \frac{100}{[A]} = \frac{39.6 \times 10^{- 3}}{2.303} = \frac{3.96 \times 10^{- 2}}{2.303} = 1.1719 \times 10^{- 2} = 0.0172 \frac{100}{[A]} = 1.040 [A] = \frac{100}{1.04} = 96.15 %

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