A certain reaction is 50% complete in 20 minutes at 300K and the same reaction is again 50% complete in 5 mins at 350K. Calculate the activation energy if the reaction is of first order.

A certain reaction is 50% complete in 20 minutes at 300K and the same reaction is again 50% complete in 5 minutes at 350K. Calculate the activation energy if the reaction is of first order.

A reaction is 50% complete in 2 hours and 75% complete in 4 hours. What is the order of the reaction?

A reaction is 50% complete in 2 hours and 75% complete in 4 hours. What is the order of the reaction?

A zero order reaction is 50% complete in 10 mins. What percentage would be completed at the end of 25 mins? In how many mins would the concentration be reduced to zero?

The rate constant of a reaction at 500K and 700K are 0.01s^-1 and 0.07s^-1 respectively. Calculate the value of activation energy for the reaction (R = 8.314 JK^-1mol^-1).

Show that in a 1st reaction, time required for completion of 99.9% is 10 times of half life time of the reaction.

In general it is observed that the rate of a chemical reaction doubles with every 10^@ rise in temperature. If the generalisation holds for a reaction in the temperature range 295K to 305K, what would be the value of activation energy for the reaction?

In a first order reaction, the concentration of the reactant is reduced from 0.6moll^(-1) to 0.2moll^(-1) in 5 minutes. Calculate the rate constant of the reaction.

The rate constants of a reaction at 500K and 700K are 0.02s^-1 and 0.07s^-1 respectively. Calculate value of activation energy for the reaction. (Given R = 8.314 JK^-1 mol^-1)

Show that for a first order reaction the time required for 75% completion is twice the time required for the completion of 50% of reaction.