Question

The gas phase decomposition of sulfuryl chloride at 600 K SO2Cl2(g)SO2(g) + Cl2(g) is first order in SO2Cl2. During one experiment it was found that when the initial concentration of SO2Cl2 was 2.83×10-3 M, the concentration of SO2Cl2 dropped to 3.06×10-4 M after 559 min had passed. Based on this experiment, the rate constant for the reaction is min-1.

Answer 1

Answer: The rate constant for the reaction is
`3.96* 10^(-3)min^(-1)`

Step-by-step explanation:

Expression for rate law for first order kinetics is given by:

`t=(2.303)/(k)\log(a)/(a-x)`

where,

k = rate constant

t = age of sample = 559 min

a = let initial amount of the reactant =
`2.83* 10^(-3)`

a - x = amount left after decay process =
`3.06* 10^(-4)`

`559min=(2.303)/(k)\log(2.83* 10^(-3))/(3.06* 10^(-4))`

`k=(2.303)/(559)\log(2.83* 10^(-3))/(3.06* 10^(-4))`

`k=3.96* 10^(-3)min^(-1)`

The rate constant for the reaction is
`3.96* 10^(-3)min^(-1)`