Half life of a first order reaction \(A(aq.) \rightarrow2B\) (aq.) is "40" min at \(27^{o}C\) and "20" min at \(37^{o}C\).The activation energy of reaction is (ln2=0.7,R=2.0 cal \(mol ^{-1}K^{-1}\)

Half life of a first order reaction A (aq.) rarr 2B (aq.) is 40 min at 27^(@)C and 20 min at 37^(@)C The activation energy of reaction is (ln2 = 0.7 , R = 2.0 cal mol ^(-1)K^(-1) )

75% of a first order reaction occurs in 30 min at 27^(@)C . 87.5% of the same reaction occurs in 30min at 57^(@)C . The activation energy of reaction is: [In 2=0.7, In 3=1.1]

A first order reaction is 50% completed in 20 minutes at 27^(@)C and in 5 min at 47^(@)C . The energy of activation of the reaction is

If the half-lives of the first order reaction at 350 K and 300 K are 2 and 20 seconds respectively, the activation energy of the reaction in kJ "mol"^(-1) is :

Calculate half life period for a first order reaction having k= 4min^(-1)

A first order reaction is 50% completed in 40 minutes at 300 K and in 20 minutes at 320 K. Calculate the activation energy of the reaction . (Given : log 2 = 0.3010 , log 4 = 0.6021 , R = 8.314 J K^(-1) mol^(-1) ) .