The activation energy of reaction is equ...

The activation energy of reaction is equal to

Threshold energy for the reaction

Threshold energy + Energy of the reactants

Threshold energy - Energy of the reactants

Threshold energy + Energy of the products.

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Activation energy=Threshold energy - Normal energy of reactants.

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Each question contains STATEMENTS-1 (Assertion) and STATEMENT -2 (Reason). Examine the statements carefully and mark the correct answer according to the instructions given below: STATEMENT -1: If the activation energy of reaction is zero, temperature will have no effect on the rate constant. STATEMENT-2: Lower the activation energy faster is the raction.

Rate constant for a chemical reaction taking place at 500K is expressed as K=A. e^(-1000) The activation energy of the reaction is :

At 27^@C in the presence of a catalyst, the activation energy of a reaction is lowered by 10 kJ mol^-1 . The ratio of log k (catalyst)/k (uncatalysed) is

The activation energy of a reaction is 56.2 kJ/mol. The ratio of the rate constant at 300 K and 305 K is (R = 8 J "mole"^(-1)K^(-1) ) about :

The activation energy of a reaction can be determined by

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.

A hydrogenation reaction is carried out at 500 K . If the same reaction is carried out in the presence of a catalyst at the same rate, the temperature required is 400 K . Calculate the activation energy of the reaction if the catalyst lowers the activation barrier by 20 kJ mol^(-1) . a) 100 kJ/mol b) 80 kJ/mol c) 60 kJ/mol d) none of these

The activation energy for the reaction if k = A is

The activation energy of the reaction, A+BtoC+D+38 kcal is 20 kcal. What would be the activation energy of the following reaction. C+DtoA+B

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