The following data were obtained during the first order thermal decomposition of SO₂ Cl₂ at constant volume.
SO₂ Cl₂ (g) → SO₂ (g) + Cl₂ (g)

Experiment

Time/s^-1

Total pressure/atm

1

0

0.5

2

100

0.6

Calculate the rate of reaction when total pressure is 0.65 atm.

Solution

we have give the data

K = \frac{2.303}{t} \log \frac{p_{1}}{p_{2}} = \frac{2.303}{100} \times \log \frac{0.5}{0.6} or K = 2.23 \times 10^{- 3} 5^{- 1}

Rate of reaction =

7.8 \times 10^{- 4} atm s^{- 1}

Some More Questions From Chemical Kinetics Chapter

For Daily Free Study Material Join wiredfaculty