Activation energy is defined as:
- AThe amount of energy to be added to the actual energy of a molecule so that the threshold energy is reached
- BThe amount of energy the molecule must contain so that it reacts
- CThe energy which a molecule should have in order to enter into an effective collision
- DThe average kinetic energy of the molecule
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Similar Questions
The rate constant for the reaction,$COCl_{2(g)} \longrightarrow CO_{(g)} + Cl_{2(g)}$ is given by $\ln[k / (min^{-1})] = -11067 / T(K) + 31.33$. The temperature at which the rate of this reaction will be doubled from that at $25^{\circ} C$ is $..... \, ^{\circ} C$.
MediumKVPY 2009
View SolutionFor a chemical reaction,the rate of reaction doubles when the temperature increases by $10\,^oC$. If the temperature is increased from $10\,^oC$ to $100\,^oC$,the rate of reaction will increase by a factor of .....
Medium
View SolutionThe rate of a reaction doubles when its temperature changes from $300 \, K$ to $310 \, K.$ Activation energy of such a reaction will be .......... $kJ \, mol^{-1}$. $(R= 8.314 \, J \, K^{-1} \, mol^{-1}$ and $\log 2=0.301)$
DifficultJEE MAIN 2013
View SolutionWhich one of the following given graphs represents the variation of rate constant $(k)$ with temperature $(T)$ for an endothermic reaction?
If the activation energy of a reaction is $80.9 \, kJ \, mol^{-1}$,the fraction of molecules at $700 \, K$,having enough energy to react to form products is $e^{-x}$. The value of $x$ is ....... . (Rounded off to the nearest integer) $[$Use $R = 8.31 \, J \, K^{-1} \, mol^{-1}]$
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