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 value of k for a reaction is 2.96 xx 10^(-30)s^(-1) . What is the order of reaction ?

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.

The rate constant of a reaction is 1.5 xx 10^7 sec^(-1) at 50^@ C and 4.5 xx 10^7 sec^(-1) at 100^@ C . Calculate energy of the activation for the reaction.

The value of k for a reaction is 2.96xx10^(30)s^-1 , what is the order of the reaction?

The rate constant of a reaction is 1.2 xx10^-3 sec^-1 at 30^@C and 2.1xx10^-3 sec^-1 at 40^@C . Calculate the energy of activation of the reaction.

The rate constant for a reaction is found to be 1.96xx10^-2 s^-1 at 313K. The activation energy of the reaction is 93.62 kJ mol^-1 . Calculate the frequency factor ,A.

The first order rate constant for the decomposition of ethyl iodide by the reaction C_2H_5I(g) rarr C_2H_4 (g) + HI(g) at 600K is 1.60 x 10^(-5) s^(-1) . Its energy of activation is 209 kJ/mol. Calculate the rate constant of the reaction at 700K.

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

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 ?

The rate constant for a reaction is 1.6 xx10^-5 and 6.36 xx 10^-3 s^-1 at 600 K and 700 K respectively. Calculate the activation energy for the reaction.