Chemical Kineti...

The rate constant of a reaction at temperature 200 $$ \mathrm{K}  $$ is10 times less than the rate constant at 400 $$ \mathrm{K}  $$ . What is theactivation energy $$ \left(E_{\mathrm{a}}\right)  $$ of the reaction $$ (R= $$ gas constant)?

For a reaction $$A \longrightarrow B+C$$ , it was found that at the end of 10 minutes from the start the total optical rotation of the system was $${ 50 }^{ o }$$ and when the reaction is complete, it was $${ 100}^{ o }$$. Assuming that only B and C are optically active and dextrorotatory. Calculate the rate constant of this first order reaction.

From the above figure, the activation energy for the reverse reaction would be:

for a zero order reaction-

For a first order reaction velocity constant is $$K={ 10 }^{ -3 }{ s }^{ -1 }$$,Two third life for it would be

The half life period for catalytic decomposition of $$  A B_{3}  $$ at $$ 50   \mathrm{mm}  $$ is found to be $$4 hrs$$ and at $$100 \mathrm{mm}  $$ it is $$2hrs$$. The order of reaction is -

Which one of the following formula represents a first-order reaction? 

A graph plotted between log $$t_{50\%}$$ vs log of concentration is a straight line. What conclusion can you draw from the given graph?

According to molecular collision theory, the reaction is subjected to:

The reactions having very high values of energy of activation are generally________