Rate Equation

In a first-order reaction, the concentration of reactant decreases from $\text{800}{\text{ mol/dm }}^3{\text{ to 50 mol/dm }}^3$ in$2 \times {10}^2 \mathrm{s}$. The rate constant of reaction in ${\mathrm{s}}^{-1}$ is

Consider a reaction $a\text{G}+\text{bH}\to \text{products}$.  When concentration of both the reactants G and H is doubled, the rate increases by eight times. However, when concentration of G is doubled keeping the concentration of H constant, the rate is doubled. The overall order of the reaction is:

Consider a reaction $a\text{G}+\text{bH}\to \text{products}$.  When concentration of both the reactants $\mathrm{G}$ and $\mathrm{H}$ is doubled, the rate increases by eight times. However, when the concentration of $\mathrm{G}$ is doubled, keeping the concentration of $\mathrm{H}$ constant, the rate is doubled. The overall order of the reaction is:

Consider the chemical reaction:

${\text{N}}_2\left(\text{g}\right)+3{\text{H}}_2\left(\text{g}\right)⟶2{\text{NH}}_3\left(\text{g}\right)$

The rate of this reaction can be expressed in terms of time derivatives of concentration of  $N_2\left(\text{g}\right)\text{ , }{\text{H}}_2\left(\text{g}\right)\text{ and }{\text{NH}}_3\left(\text{g}\right)$ Identify the correct relationship amongst the rate expressions:

Hydrogen gas, ${\mathrm{H}}_2\left(\mathrm{g}\right)$, reacts with iodine gas, ${\mathrm{I}}_2\left(\mathrm{g}\right)$, to form hydrogen iodide, $\mathrm{HI}\left(\mathrm{g}\right)$:

${\mathrm{H}}_2\left(\mathrm{g}\right) + {\mathrm{I}}_2\left(\mathrm{g}\right) \to 2\mathrm{HI}\left(\mathrm{g}\right)$

The mechanism of the two-step reaction is considered to be:

step $1$: ${\mathrm{I}}_2\left(\mathrm{g}\right) \underset{{\mathrm{k}}_{-1}}{\overset{{\mathrm{k}}_1}{\leftrightharpoons }} 2\mathrm{I}\left(\mathrm{g}\right)$                        fast

step $2$: $2\mathrm{I}\left(\mathrm{g}\right) + {\mathrm{H}}_2\left(\mathrm{g}\right) \stackrel{{\mathrm{k}}_2}{\to } 2\mathrm{HI}\left(\mathrm{g}\right)$     slow

What is the rate equation for the overall reaction?

List the properties of a catalyst.

Give the name of the catalyst that used in the contact process.

Define trimolecular reaction.

Define biomolecular reaction.

Define unimolecular reaction.

Draw a graph between rate and concentration of reactants for first order reaction.

The graph between rate and concentration of reactants for second order reaction is 

The plot of 1/[A] versus time is a straight line with k = slope of the line. Other graphs are curved for a second order reaction.

Explain second order reaction with an example ? Draw the graph between 1/A vs time for second order reaction.

The graph between rate and concentration of reactants for first order reaction is 

Draw a graph between rate and concentration of reactants for first order reaction.

For, a zero-order reaction, the plot of concentration of reactant versus rate is linear with negative slope and zero intercept.