is . kJ/mol, what will be the value of pre-exponential factor. . Consider a certain reaction A ® Products with k = .
× – s – . Calculate the concentration of A remaining after s if the initial concentration of A is . mol L – . .
Sucrose decomposes in acid solution into glucose and fructose according to the first order rate law, with t / = . hours. What fraction of sample of sucrose remains after hours ? .
The decomposition of hydrocarbon follows the equation k = ( . × s – ) e -28000 K / T Calculate E a . . The rate constant for the first order decomposition of H O is given by the following equation: log k = .
– . × K / T Calculate E a for this reaction and at what temperature will its half-period be minutes? . The decomposition of A into product has value of k as .
× s – at ° C and energy of activation kJ mol – . At what temperature would k be . × s – ? .
The time required for % completion of a first order reaction at 298K is equal to that required for its % completion at 308K. If the value of A is × s – . Calculate k at 318K and E a . .
The rate of a reaction quadruples when the temperature changes from K to K. Calculate the energy of activation of the reaction assuming that it does not change with temperature. Answers to Some Intext Questions . r av = .
× – Ms – . Rate of reaction = rate of diappearance of A = . mol litre – min – . Order of the reaction is .
. X ® Y Rate = k [X] The rate will increase times . t = s . .