Rate constant `k = 1.2 xx 10^(3) mol^(-1) L s^(-1)` and `E_(a) = 2.0 xx 10^(2) kJ mol^(-1)`. When `T rarr oo`:

Identify the reaction order form each of the following rate constants: a. k = 7.06 xx 10^(-3) mol L^(-1) s^(-1) b. k = 5.6 xx 10^(-5) s^(-1) c. k = 1.25 xx 10^(-2) mol^(-1)l s^(-1) d. k = 1.25 xx 10^(-2) mol L^(2)s^(-1) e. k = 5.0 xx 10^(-6) atm^(-1)s^(-1)

Identify the reaction order form each of the following rate constants: a. k = 7.06 xx 10^(-3) mol L^(-1) s^(-1) b. k = 5.6 xx 10^(-5) s^(-1) c. k = 1.25 xx 10^(-2) mol^(-1)l s^(-1) d. k = 1.25 xx 10^(-2) mol L^(2)s^(-1) e. k = 5.0 xx 10^(-6) atm^(-1)s^(-1)

For the reaction: [Cr(H_(2)O)_(6)]^(3) + [SCN^(ɵ)] rarr [Cr(H_(2)O)_(5)NCS]^(2+)H_(2)O The rate law is r = k[Cr(H_(2)O)_(6)]^(3+)[SCN^(ɵ)] . The value of k is 2.0 xx 10^(-6) L mol^(-1) s^(-1) at 14^(@)C and 2.2 xx 10^(-5) L mol^(-1)s^(-1) at 30^(@)C . What is the value of E_(a) ?

For the reaction: [Cr(H_(2)O)_(6)]^(3) + [SCN^(ɵ)] rarr [Cr(H_(2)O)_(5)NCS]^(2+)H_(2)O The rate law is r = k[Cr(H_(2)O)_(6)]^(3+)[SCN^(ɵ)] . The value of k is 2.0 xx 10^(-6) L mol^(-1) s^(-1) at 14^(@)C and 2.2 xx 10^(-5) L mol^(-1)s^(-1) at 30^(@)C . What is the value of E_(a) ?

The rate constant for two parallel reactions were found reactions were found to be 1.0 xx 10^(–2)" dm"^(3)" mol"^(-1) s^(–1) and 3.0 xx 10^(–2)" dm"^(3)" mol"^(–1) s^(–1) . If the corresponding energies of activation of the parallel reactions are 60.0" kJ mol"^(–1) and 70.0" kJ mol"^(–1) respectively, what is the apparent overall energy of activation ?

Identify the reaction order from each of the following rate constants. (i) k = 2.3 xx 10^(-3) L mol^(-1)s^(-1) (ii) k = 3 xx 10^(-1)s^(-1)