Exercise 1

For a chemical reaction, $\mathrm{A}+\mathrm{B}\to \mathrm{Products}$, the order is one with respect to each A and B. Value of x and y from the given data is :

Why do colliding molecules have activation energy?

A first-order reaction takes $69.3 \min$ for $50\%$ completion. What is the time needed for $80\%$ of the reaction to get completed?

Select the correct statements out of I, II and III for a zero order reaction:

I. Quantity of the product formed is directly proportional to time.

III. If $50\%$ reaction takes place in $100$ minutes, $75\%$ reaction will take place in $150$ minutes.

III.Larger the initial concentration of the reactant, greater is the half-life period.

For a certain reaction $\mathrm{X}$, rate $= 0.7{\mathrm{Z}}_{\mathrm{AB}}\mathrm{e}{ }^{-\mathrm{E}{ }_{\mathrm{A}} /\mathrm{RT}}$ .

It is seen that for another reaction, $\mathrm{Y}$, rate = ${\mathrm{Z}}_{\mathrm{AB}}\mathrm{e} -\mathrm{E}{{ }_{\mathrm{A} }}^{/\mathrm{RT}}$ .

Based on the above, what can be said about reactions X and Y?

For the reaction, ${\mathrm{NO}}_2\left(\mathrm{g}\right)+\mathrm{CO}\left(\mathrm{g}\right)⟶{\mathrm{CO}}_2\left(\mathrm{g}\right)+\mathrm{NO}\left(\mathrm{g}\right)$, the experimentally determined rate expression below $400 \mathrm{K}$ is: rate $=\mathrm{k}{\left[{\mathrm{NO}}_2\right]}^2$. What mechanism can be proposed for this reaction?

Arrhenius equation can be represented graphically as follows:

The (i) intercept and (ii) slope of the graph are:

For the reaction, $\mathrm{A}+2\mathrm{B} \to {\mathrm{AB}}_2$, the order w.r.t. reactant $\mathrm{A}$ is $2$ and w.r.t. reactant $\mathrm{B}$ is zero. What will be change in rate of reaction if the concentration of $\mathrm{A}$ is doubled and $\mathrm{B}$ is halved?