Chemical Kineti...

For a first order reaction, the ratio of the time taken for $$7/8^{th}$$ of the reaction to complete to that of half of the reaction to complete is :

A first order reaction is $$50$$% complete in $$30$$ minutes at $$27^{\circ}C$$ and in $$10$$ minutes at $$47^{\circ}C$$. The reaction rate constant at $$27^{\circ}C$$ and the energy of activation of the reaction are respectively.

Threshold energy is equal to:

In the reaction, $$2NO+Cl_2\rightarrow 2NOCl$$, it has been found that doubling the concentration of both the reactants increases the rate by a factor of eight but doubling the chlorine concentration alone only doubles the rate. Which of the following statements is incorrect?

The rate constant is given by the equation $$k = P.Ze^{-E_{a}/RT}$$. Which factor should register $$a$$ decrease for the reaction to proceed more rapidly:

Fill up the following with suitable terms.

For an elementary bi-molecular reaction of the type $$A + B \rightarrow C$$ activation energy is equal to 20 Kcal. If specific rate of reaction at 500 K is 4.2 $$\times$$ $$10^{-3}M^{-1}sec^{-1}$$, then identify the incorrect option(s). [Given : ln ($$2.1 \times$$ $$10^{-9}$$) = - 20] 

The activation energy for the forward reaction X Y is $$60$$ KJ $$mol^{-1}$$ and $$\Delta H$$ is $$-20$$ KJ $$mol^{-1}$$. The activation energy for the backward reaction Y X is:

The half-life of a first-order reaction is $$100$$ seconds. What is the time required in seconds for $$90\%$$ completion of the reaction?