The reaction A `rarr` B+C shows the result given show that it is a fist order reaction-

plot a graph of reaction -rate vs concentration of the reactant for a fist order reaction.

If a reaction A+B rarr C is exothermic to the extent of 30 kJ/mol and the forward reaction has an activation energy 70 kJ/mole. The activation energy for the reverse reaction is

What will be the nature of the graph showing the concentration of the reactant and time of a first order reaction ?

On the basis of rate equation show that a fist order reaction does never go to completion. For an elementary reaction A + B rarr C , the rate constant increases 10 times on increasing the temperature from 27^@C by 10 degrees, Find out the activation energy of the reaction.

For a reaction A+B rarr C consider the following data:

On the basis of rate equation show that a first order reaction does never go to completion.

In hypothetical reaction A_2+B_2 = 2AB follows the mechanism as given below: A_2 iff A+A (fast reaction) A+B_2 to AB+B (slow reaction) A+B to AB (fast reaction) give the rate law and order of reaction.

In the reaction: ArarrB+C , the rate of formation of C becomes twice if the concentration of A is made double. What is the order of the reaction ?