Chemical Kineti...

If the order of the reaction $$x+y\xrightarrow[]{hv}xy$$ is zero, it means that the rate of ____

Which the following statements is true for a first order reaction?

Fill in the blanks by choosing the correct option:

Cyclopropane rearranges to form propene
$$ \Delta \rightarrow CH_3 -CH =CH_2 $$
this follows first order kinetics. the rate constant is $$ 2.714 \times 10^{-3} sec^{-1} $$the initial concentration of cyclopropane is $$ 0.29 M $$what will be concentration  of cyclopropane after 100 sec ?

the half - life of the reaction $$ X \rightarrow Y $$ following first  order kinetics , when the initial concentration of X is $$ 0.01 mol L^{-1} $$ and initial rate is $$ 0.00352 mol L^{-1} min^{-1} $$ will be 

the rate constant for a first order reaction is $$ 2 \times 10^{-2} min^{-1} $$ the half -life period of reaction is 

Rate constant in case of first order reaction is 

Which of the following is incorrect statement ?

The activation energy of the reaction, $$A + B \rightarrow C + D + 38kcal$$ is $$20$$ kcal, What would be the activation energy of the reaction,
$$C + D \rightarrow A + B$$

In a certain first-order reaction, $$B^{n+}$$ is getting converted to $$B^{(n+4)+}$$  in solution. The rate constant of this reaction is measured by titrating a volume of the solution with a reducing agent which reacts only with $$B^{n+}$$ and $$B^{(n+4)+}$$. In the process, it converts  to $$B^{n+}$$ to $$B^{(n-2)+}$$ and $$B^{(n+4)+}$$ to $$B^{(n-1)+}$$,At $$t=0$$ the volume of reagent consumed is 55 ml and at $$t = 20$$ min, the volume used is 70.5 ml. The rate constant for the conversion of $$B^{n+}$$ of $$B^{(n+4)+}$$ (ln 2 = 0.7, ln 5 = 1.6)