If the reaction rate for chemical reaction be `5.4xx10^(-4) s^(-1)` at `25^@C` then at what temperature it will be `4.2xx10^(-2)S^(-1)`? Give `E_a=376k.J mol^(-1)` `N_2O_5 (g) rarrNO_2+O_2` Dissociation of `N_2O_5` is a 1st order reaction.

The rate of a reaction is 1.2xx10^-3 L mol^-1s^-1 , What is the order of the reaction?

The specific reaction rates of a chemical reaction are 2.45xx10^(-5)sec^(-1)" at "273K and 16.2 xx10^(-4) sec^(-1) at 303 K. Calculate the activation energy.

Identify the reaction order from the following rate constants. k= 2.3 xx 10^-5 Lmol^-1 s^-1

The rate constant of a reaction 1.5xx10^(7)s^(-1) " at " 50^(@)C and 4.5xx10^(7)s^(-1) at 100^(@)C Evaluate the Arrhenius parameters A and E_(a)

The rate constant of a chemical reaction at 600K is 1.6xx10^(-5)s^(-1) . The activation energy of the reaction is 209"kJ.mol"^(-1) . Calculate its rate constant at 700K.

Identify the reaction order from each of the given rate constants: k=2.3xx10^(-5)"L.mol"^(-1).s^(-1)

Specific reaction rates for a reaction at 300K and 310K are 3xx10^(-6) S^(-1) and 2.8xx10^(-5 S^(-1 . Calculate the activation enrgy for that reaction.

At a particular temperature , the rate constant of the reaction 2N_(2)O_(5)(g)rarr4NO_(2)(g)+O_(2)(g) " is "6xx10^(-5)s^(-1) . If the reaction -rate of the reaction is 4.2xx10^(-5)"mol.L"^(-1).s^(-1) , then concentration of N_(2)O_(5)("mol.L"^(-1)) will be -

The initial rate of a first order reaction is 5.2 xx 10^(-6)" mol.lit"^(-1).s^(-1) at 298 K. When the initial concentration of reactant is 2.6xx10^(-3)" mol.lit"^(-1) , calculate the first order rate constant of the reaction at the same temperature.

If the rate of reaction is 2.6xx10^-3 mol L^-1s^-1 at 50^@C and 7.02xx10^-2 mol L^-1s^-1 at 80^@C : then what will be the temperature coefficient of the reaction ?