Chemical Kineti...

Find the values of $$A, B$$ and $$C$$ in the following table for the reaction $$X + Y\rightarrow Z$$. The reaction is of first order w.r.t $$X$$ and zero w.r.t. $$Y$$.

The energy diagram of a reaction $$P + Q \rightarrow R + S$$ is given. What are $$A$$ and $$B$$ in the graph?

The activation energy for the reaction-
$$H_{2}O_{2} \rightarrow H_{2}O + \dfrac {1}{2} O_{2}$$
is $$18\ K\ cal/mol$$ at $$300\ K$$. calculate the fraction of molecules of reactants having energy equal to or greater than activation energy?
Anti log $$(-13.02) = 9.36\times 10^{-14}$$

The following data were obtained during the first order thermal composition of $$SO_{2}Cl_{2}$$ at a constant volume.
$$SO_{2}Cl_{2(g)} \rightarrow SO_{2(g)} + Cl_{2(g)}$$

How much faster would a reaction proceed at 298 K than at 273 K, if the activation energy is $$65 kJ mol^{-1}$$?

The reaction at hydrogen and iodine monochloride is represented by the equation is
$$H_{2} (g) + 2ICl (g) \rightarrow 2HCl (g) + I_{2} (g)$$
This reaction is first order in $$H_{2}(g)$$ and also first - order in ICI(g). which of these proposed mechanism can be consistent with the given information about this reaction ?
Mechanism I : $$H_{2} (g) + 2ICl (g) \rightarrow 2HCl (g) + I_{2} (g)$$
Mechanism II : $$H_{2} (g) + ICl (g) \overset{slow}{\rightarrow} HCl (g) + HI (g)$$
$$HI (g) + ICl (g) \overset{fast}{\rightarrow} HCl (g) + I_{2} (g)$$ :

The activation energy for a reaction is $$9.0 k cal/mol$$. The increase in the rate constant when its temperature is increased from $$298 K$$ to $$308 K$$ is:

For a reaction $$A_{2} + B_{2}\rightleftharpoons 2AB$$ the figure shows the path of the reaction in absence and presence of a catalyst. What will be the energy of activation for forward $$(E_{f})$$ and backward $$(E_{b})$$ reaction in presence of a catalyst and $$\triangle H$$ for the reaction? the dotted curve is the path of reaction in presence of a catalyst.

The fraction of collisions that posses the energy $$E_a$$ is given by:

For an exothermic reaction $$A \rightarrow B$$, the activation energy is $$65\ kJ\ mol^{-1}$$ and heat of reaction $$-42\ kJ\ mol^{-1}$$. The activation energy for the reaction $$B \rightarrow A$$ would be :-