What type of reactions are represented by following equation : 2KClO3 → 2KCl + 3O2

Explanation

Let first calculate `k_1 and k_2` at temperature 300 K and 350 K
At 300 k `t_(1/2) = 0.693/k ` (Half Life Equation)
`k = (0.693)/(t_(1/2))`
`k_1 = 0.693/20`
At 350 K `t_(1/2) = 5`
so, `k_2 = (0.693)/(t_(1/2))`
so ,` k_2 = (0.693)/(5)`
Now According to Arrhenius eqn.
`log (0.693)/5 xx 20/0.693 = (E_a)/(2.303 xx 8.314)[1/300 - 1/350]`
`0.602 = (E_a xx 50)/(2.303 xx 8.314 xx 300 xx 350)`
`E_a = (0.602 xx 2.303 xx 8.314 xx 300 xx 350)/(50)`
`E_a = 24206 J mol^(-1)`