The Rate Law and Rate Constant

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?

For a given reaction $3\mathrm{A}\mathrm{ }+\mathrm{B}\to \mathrm{C}+\mathrm{D}$ the rate of reaction can be represented by

The units of rate constant is same as that of rate. The order of the reaction is:

Rate law cannot be determined from balanced chemical equation if _____.

What is a rate constant?

Rate law cannot be determined from balanced chemical equation if _______.

The rate of reaction, $\mathrm{A}\to$ Products is $1.25\times {10}^{-2}\mathrm{M}/\mathrm{s}$ when concentration of $\mathrm{A}$ is $0.45\mathrm{M}$. Determine the rate constant if the reaction is second order in $\mathrm{A}$.

The following results were obtained in the decomposition of H2O2 in KI solution at 30°C

Show that the reaction is first order. Calculate the rate constant of the reaction.

From the following data for the liquid phase reaction $\mathrm{A} \to \mathrm{B}$, determine the order of the reaction and calculate its rate constant.

A reaction is first order with respect to reactant $\mathrm{A}$ and second order with respect to reactant $\mathrm{B}$. The rate law for the reaction is given by

For the reaction, ${\mathrm{A}}_2+\mathrm{B}+\mathrm{C}⟶\mathrm{AC}+\mathrm{AB},$ it is found that tripling the concentration of ${\mathrm{A}}_2$ triples the rate, doubling the concentration of $\mathrm{C}$ doubles the rate and doubling the concentration of $\mathrm{B}$ has no effect.

Why the change in concentration of $\mathrm{B}$ has no effect?

For the reaction, ${\mathrm{A}}_2+\mathrm{B}+\mathrm{C}⟶\mathrm{AC}+\mathrm{AB},$ it is found that tripling the concentration of ${\mathrm{A}}_2$ triples the rate, doubling the concentration of $\mathrm{C}$ doubles the rate and doubling the concentration of $\mathrm{B}$ has no effect.

What is the rate law?

Comment on the relationship between coefficients of the balanced overall equation for a reaction and the exponents to which the concentration terms in the rate law are raised. What do these exponents represent?

Write the rate law for the following reaction:
A reaction that is second order in $\mathrm{NO}$ and first order in ${\mathrm{Br}}_2.$
 

For the reaction $2\mathrm{A} + \mathrm{B} \to$ products, find the rate law from the following data

What is the rate constant and order of the reaction?
 

Consider the reaction $2\mathrm{A} + 2\mathrm{B} \to 2\mathrm{C} + \mathrm{D}$. From the following data, calculate the order and rate constant of the reaction.

Write the rate law of the reaction.