Chemical Kineti...

A reaction takes place in thee steps.The rate constants are $$K_1,K_2$$ and $$k_3$$. The over all rate constant $$k=\cfrac{K_1K_3}{K_2}$$. If (energy of activation) $$E_1, E_2$$ and $$E_3$$ are $$100, 20$$ and $$40 kJ$$.The overall energy of activation is:

In a reaction carried out at 400 k, $$0.0001\%$$ of the total number of collisions are effective. The energy of activation of the reaction is:

What is the activation energy for a reaction if its rate doubles when the temperature is raised from $$20^{\circ}C$$ to $$35^{\circ}C$$?

At a certain temperature, the first order rate constant $$k_{1}$$ is found to be smaller than the second order rate constant $$k_{2}$$. If $$E_{a}(1)$$ of the first order reaction is greater than $$E_{a}(2)$$ of the second order reaction, then as temperature is raised:

For the following reaction at a particular temperature, according to the equations,
$$ 2N_2O_5 \rightarrow 4NO_2 + O_2 $$ 
$$2NO_2+1/2O_2 \rightarrow N_2O_5$$
the activation energies are $$E_1$$ and $$E_2$$ respectively, then:

A substance $$A$$ undergoes decomposition in solution following the first order kinetics. Flask $$I$$ contains 1 litre of 1 M solution of $$A$$ and flask $$II$$ contains $$100$$ $$ml$$ of 0.6 M solution. After 8 hours, if the concentration of $$A$$ in flask $$I$$ became 0.25 M, what will be the time required in hours for the concentration of $$A$$ in flask $$II$$ to become 0.3 M?

It takes $$1\ h$$ for a first order reaction to go to $$50$$% completion. The total time required for the same reaction to reach $$87.5$$% completion will be:

Calculate the rate constant for decomposition of ammonium nitrate from the following data;
$$NH_4NO_2\rightarrow N_2+2H_2O$$

The spontaneous decomposition of radio nuclei is a first order rate process.U-238 disintegrates with the emission of $$\alpha$$-particles and has a half-life of $$4.5 \times 10^9$$ years. If at time t=0, 1 mole of U-238 is present, what will be the number of nuclei left after 1 billion years?

For the equilibrium, $$A(g) \rightleftharpoons B(g), \triangle H$$ is $$-40\ kJ/mol$$. If the ratio of the activation energies of the forward $$(E_{f})$$ and reverse $$(E_{b})$$ reactions is $$2/3$$ then: