The rate constant of a first order reaction, Given that the activation energy of the reaction is 28 kJ mol-1 and assuming Arrhenius behavior for the temperature dependence, the total time required to obtain 90% of Y at 350 K is_____________ s. (Up to one decimal place. Use R = 8.31 J K-1 mol-1 )Correct answer is '280 to 300'. Can you explain this answer?

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The rate constant of a first order reaction,

Given that the activation energy of the reaction is 28 kJ mol^-1 and assuming Arrhenius behavior for the temperature dependence, the total time required to obtain 90% of Y at 350 K is_____________ s. (Up to one decimal place. Use R = 8.31 J K^-1 mol^-1)

Correct answer is '280 to 300'. Can you explain this answer?

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The rate constant of a first order reaction, Given that the activation energy of the reaction is 28 kJ mol-1 and assuming Arrhenius behavior for the temperature dependence, the total time required to obtain 90% of Y at 350 K is_____________ s. (Up to one decimal place. Use R = 8.31 J K-1 mol-1 )Correct answer is '280 to 300'. Can you explain this answer?

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