The decomposition of hydrocarbon follows the equation `k = (4.5 × 10^(11) S^(-1)) e^(-28000K/T)` Calculate `E_a`

The rate constant for the first order decomposition of H_2O_2 is given by the following equation: log k = 14.34 - 1.25 × 10^4K/T Calculate E_a for this reaction and at what temperature will its half-period be 256 minutes?

A substance undergoes first order decomposition. The decomposition follows we parallel first order reactions as : k_1= 1.26 xx 10^-4 s^-1 k_2= 3.8 xx 10^-5 s^-1 The percentage distribution of B and C are

The rate constant for the decomposition of hydrocarbons is 2.418 xx 10^(-5)s^(-1) at 546 K. If the energy of activation is 179.9 kJ/mol, what will be the value of pre-exponential factor.

Complete the following equation : MnO_4^(-)+ 8H^(+)+ 5e^(-) rarr

Identify the reaction order from each of the following rate constants. k = 3 xx 10^(-4) s^(-1)

The time required for 10% completion of a first order reaction at 298K is equal to that required for its 25% completion at 308K. If the value of A is 4 × 10^(10) s^(-1) . Calculate k at 318K and E_a .

The decomposition of A into product has value of k as 4.5 xx 10^3 s^-1 at 10°C and energy of activation 60 kJ mol^-1 . At what temperature would k be 1.5 xx 10^4 s^-1 ?

The decomposition reaction of ammonia gas on platinum surface has a rate constant, k = 2.5xx 10^-4 mol L^-1 s^-1 . What is the order of the reaction ?