Question

The rate of reaction increases by 2 times when the temperature of the reaction raised from 300k to 310k calculate the energy of activation of the reaction

Answer 1

Answer:

The amount of increase is dependent on the activation energy. For a very low activation energy, there will be almost no change (this is what you obtained by removing EaEa and TT). For a high activation energy, the change will be quite large. For example, with an activation energy of 110kJmol110kJmol, you the rate will increase by about 1616 times.

exp(−EaR∗320)exp(−EaR∗300)=exp(−111000J8.314∗320)exp(−111000J8.314∗300)=7.6×10−194.7×10−20=16.14exp⁡(−EaR∗320)exp⁡(−EaR∗300)=exp⁡(−111000J8.314∗320)exp⁡(−111000J8.314∗300)=7.6×10−194.7×10−20=16.14

So there really isn't an "in general" answer. However, many text books give a crude estimate that the rate will double when the temperature is increased by 1010. This isn't in general the case, as it depends on the temperature range (a change from 300300 to 320320 is more significant that a change from 600600 to