প্রতিক্রিয়ার হার দ্বিগুণ হয় যখন এর তাপমাত্রা পরিবর্তন করে `300 K` থেকে `310 K` হয়।

For a reaction, E_(a)= 0 and k= 3.2xx10^(4)s^(-1) at 300 K . The value of k at 310 K would be

Half life of a first order chemical reaction is 69 hr at 300 K. Also , rate of this reaction is doubled as temperature is increased from 300 K to 310 K. Determine activation energy and pre - exponential factor for this reaction.

Activation energy of reactions for which rate constant is doubled when the temperature is increased by 10^(@) (from 300 K to 310 K) is nearly………………… .

The molar heat capacities at constant pressure (assumed constant with respect to temperature) at A, B and C are in ratio of 3:1.5:2.0 The enthalpy change for the exothermic reaction A + 2B rarr 3C at 300 K and 310 K is DeltaH_(300) "and" DeltaH_(310) respectively then:

The rate of a reaction doubles when the tempeature changes from 300 K to 310 K. Activation energy for the reaction is: (R = 8.314 JK^(-1) mol^(-1), log2 = 0.3010)

The rate constant of a reaction increases by 7% when its temperature is raised from 300 K to 310 K, while its equilibrium constant increases by 3%. Calculate the activation energy of the forward and reverse reactions.

The rate of a reaction doubles when its temperature changes form 300 K to 310 K . Activation energy of such a reaction will be: (R = 8.314 JK^(-1) mol^(-1) and log 2 = 0.301)