Chemical Kineti...

The initial rate of zero-order reaction of the gaseous reaction $$A(g)\rightarrow2B(g)$$ is $$10^{-2}M min^{-1}$$. If the initial concentration of A is 0.1 M, then the concentration of B after 60 sec would be:

In the following reaction, $$ A\rightarrow B$$, rate constant is $$1.2\times10^{-2} Ms^{-1}$$. What is the concentration of $$B$$ after $$10$$ min, if we start with $$10\ M$$ of $$A$$?

To initiate a reaction, minimum energy which is required to break bonds is called

1. bond energy
2. activation energy
3. breaking energy
4. ionization energy

Radioactive disintegration follows _____ order kinetic.

For the first-order reaction $$A\rightarrow product$$s, the half-life is $$200$$s. The rate constant of the reaction is:

For a first order reaction $$A\rightarrow B$$ the rate constant is $$x\ min^{−1}$$ . If the initial concentration of A is 0.01M , the concentration of A after one hour is given by the expression:

The decomposition of an equal mole of two reactants P and Q obey 1st order kinetics with half-life 54 and 18 minutes respectively. If both are allowed to run for 54 minutes. The ratio of mole of Q and P left after decomposition will be:

If 'a' is the initial concentration of a substance which reacts according to zero order kinetics and K is rate constant, the time for the reaction to go to completion is:

Activation energy of a reaction is:

Calculate the partial pressure of reactants and products, when azomethane decomposed at an initial pressure of 200 mm for 30 minutes according to
$$(CH_3)_2N_2\rightarrow C_2H_6+N_2$$
The rate constant is $$2.5\times 10^{-4} sec^{-1}$$.