Question

The following data were obtained during the first order thermal decomposition of SO₂Cl₂ at a constant volume                                                                              

SO₂Cl₂(g) \(\xrightarrow[]{\ \ \ \ \ \ \ }\) SO₂(g) + Cl₂(g)

Exp	Time (Sec)	Total pressure (atm)
1	0	0.5
2	100	0.6

If rate of reaction (atm sec^–1) when total pressure is 0.65 atm is y × 10^–5 (Initially only SO₂Cl₂ is taken) then determine the value of y.

(log2 = 0.3, log3 = 0.48, log4 = 0.6, log 5 = 0.7)               

Answer 1

SO₂Cl₂(g) \(\xrightarrow[]{\ \ \ \ \ \ \ }\) SO₂(g) + Cl₂(g)

0.5                     –             –

0.5-x                  x            x

P_T = 0.5 + x = 0.6

x = 0.1

K = \(\frac{2.303}{100}\log \frac{0.5}{0.4}\) = \(\frac{2.303}{1000}\)

When tc P_T = 0.65        

x = 0.15 

Rate nj = K \([{{P}_{S{{O}_{2}}C{{l}_{2}}}}]\) = \(\frac{2.303}{1000}\) × 0.35 = 80.6 × 10^–5