Question
For the first order thermal decomposition reaction, the following data were obtained:
$\text{C}_{2}\text{H}_{5}\text{Cl}\text{(g)}\rightarrow \text{C}_{2}\text{H}_{4}\text{(g)} + \text{HCl}\text{(g)} $
Calculate the rate constant
$($Given: $\log 2 = 0.301, \log 3=0.4771, \log 4 =0.6021)$
$\text{C}_{2}\text{H}_{5}\text{Cl}\text{(g)}\rightarrow \text{C}_{2}\text{H}_{4}\text{(g)} + \text{HCl}\text{(g)} $
| Time/sec | Total pressure/atm |
| $0$ | $0.30$ |
| $300$ | $0.50$ |
$($Given: $\log 2 = 0.301, \log 3=0.4771, \log 4 =0.6021)$