Order of Reaction

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:

For the reaction $\mathrm{A}+\mathrm{B}⟶\mathrm{C}+\mathrm{D}$ the following data was collected. The order of the reaction is

Compounds $\mathrm{A}$ and $\mathrm{B}$ react according to the equation $2{\mathrm{A}}_{\left(\mathrm{g}\right)}+{\mathrm{B}}_{\left(\mathrm{g}\right)}\to 2{\mathrm{C}}_{\left(\mathrm{g}\right)}+{\mathrm{D}}_{\left(\mathrm{g}\right)}$.
The initial rate of formation was determined at different initial concentrations of$$$\mathrm{A}$ and $\mathrm{B}.$ The following results were obtained. The rate law for this reaction may be [All concentrations are in $\mathrm{mol}/\mathrm{lit}$].

A reaction has rate constant $\mathrm{k}=2.4\times {10}^{-4}{ \mathrm{s}}^{-1}.$ Then find the ratio of ${\mathrm{t}}_{99.9}$ to $t_{50}.$

If 50 % of a reaction occurs in 100 second and 75 % of the reaction occurs in 200 second, the order of this reaction is:

Which of the following is incorrect?

The rate of the haemoglobin $\left(\mathrm{Hb}\right)$-carbon monoxide reaction, 

$4\mathrm{Hb}+3\mathrm{CO}\to {\mathrm{Hb}}_4(\mathrm{CO}{)}_3$

has been studied at $20°\mathrm{C}$. The Concentration of reactants are expressed in $\mathrm{\mu } \mathrm{mole}/\mathrm{L}.$ 

The rate constant for the reaction is $7\times {10}^{-\mathrm{x}} \mathrm{L} {\mathrm{\mu mol}}^{-1}.{\sec }^{-1}$. The value of $\mathrm{x}$ is
 

Which of the following is incorrect?

The reaction between ${\mathrm{A}}_2$ and ${\mathrm{B}}_2$ follows the equation ${\mathrm{A}}_2+{\mathrm{B}}_2\to 2\mathrm{AB}$. The following data were observed:

The value of the rate constant for the given reaction is:

For the following elementary reaction, determine its order of reaction and the dimensions of the rate constant:

$2\text{NO}\left(\text{g}\right)\to {\text{N}}_2\text{O}\left(\text{g}\right)+\frac{1}{2}{\text{O}}_2$

For a reaction, $\mathrm{A}+2\mathrm{B}\to \mathrm{C}$, the rate is given by $+\frac{\mathrm{d}\left[\mathrm{C}\right]}{\mathrm{dt}}=\mathrm{k}\left[\mathrm{A}\right]\left[\mathrm{B}\right]$, hence, the order of the reaction is:

Order of a reaction with rate constant ${\text{mol}}^{-1}{\mathrm{L}}^{}{\mathrm{s}}^{-1}$ is :

The plot of concentration of a reactant vs time for a chemical reaction is shown below.

The order of this reaction with respect to the reactant is

A reaction occurs by the following mechanism:
(i) ${\mathrm{NO}}_2\left(\mathrm{g}\right)+{\mathrm{F}}_2\left(\mathrm{g}\right)\to {\mathrm{NO}}_2\mathrm{F}\left(\mathrm{g}\right)+\mathrm{F}\left(\mathrm{g}\right)$
(ii) $\mathrm{F}\left(\mathrm{g}\right)+{\mathrm{NO}}_2\left(\mathrm{g}\right)\to {\mathrm{NO}}_2\mathrm{F}\left(\mathrm{g}\right)$
The net reaction is:

Rate constant of a chemical reaction is $1.72\times {10}^{–4} {\mathrm{s}}^{–1}$. Calculate the order of reaction?

${\mathrm{t}}_{1/2}$ = constant, confirms that the order of the reaction is one.

${\mathrm{a}}^2\times {\mathrm{t}}_{1/2}$ = constant, confirms that the reaction is of: ($\mathrm{a}=$ Initial concentration).

For the reaction $\mathrm{A}+\mathrm{B}\to$ product

$\mathrm{r}=\mathrm{K}\left[\mathrm{A}{]}^{2/3}\right[ \mathrm{B}{]}^{4/3}$

order of reaction is :-

At particular concentration, the half life of the reaction is $100$ minutes. when the concentration of reactant becomes double half life becomes $25$ minutes, then what will be the order of the reaction ?

Show that the time required for $99.9\%$ completion of a first order reaction is three times the time required for $90\%$ completion.