Determination of 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 a reaction, $\mathrm{K}=4.5\times {10}^{-4}\mathrm{L}{\mathrm{mol}}^{-1}{\mathrm{s}}^{-1}$. What is order of reaction?

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

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
 

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:

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:

${\mathrm{t}}_{1/2}$ = 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).

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 ?

During kinetic studies of the reaction, the following results were obtained
$2\mathrm{A}+\mathrm{B}\to$ product
How much time (in minutes) required to consume half of $\mathrm{A} ?$

The relative concentration of two samples of same substance is 200 and 50 respectively and their half-lives are 0.1 and 0.4 s respectively. What is the order of reaction?

For the reaction. $\mathrm{A}+2\mathrm{B}⟶\mathrm{C}$, the reaction rate is doubled if the concentration of $\mathrm{A}$ is doubled. The rate is increased by four times when the concentrations of both $\mathrm{A}$ and $\mathrm{B}$ are increased by four times. The order of the reaction is......

Which of the following is second-order reaction?
 

Example of a second order reaction among the following is:

At a temperature of $500\mathrm{ }\mathrm{K}$, the half-life period of a gaseous reaction at an initial pressure of $80\mathrm{ }\mathrm{k}\mathrm{P}\mathrm{a}$ is $350\mathrm{ }\mathrm{s}$. What is the order of the reaction, if the pressure is $40\mathrm{ }\mathrm{k}\mathrm{P}\mathrm{a}$, the half-life period changes to $175\mathrm{ }\mathrm{s}$? 

For a reaction between $\mathrm{A}$ and $\mathrm{B}$, the rate law is given by $\text{k}{\left[\text{A}\right]}^{\text{n}}{\left[\text{B}\right]}^{\text{m}}$. If we double the concentration of $\mathrm{A}$ and half the concentration of $\mathrm{B}$, the ratio of the new rate to the earlier rate of reaction will be:

Consider the following reaction:

$2\mathrm{A}+\mathrm{B}\to \mathrm{product}$

The half-life of reaction did not change when concentration of B alone was doubled. The rate increased by two times when the concentration of A alone was doubled. What is the unit of rate constant for above reaction?

Consider the reaction : $\mathrm{A}\left(\mathrm{g}\right)\to \mathrm{B}\left(\mathrm{g}\right)$

If the time taken for the partial pressure of gas A to fall from $1.0 \mathrm{atm}$ to $0.5 \mathrm{atm}$ is $10 \mathrm{seconds}$ and  $\text{from }0.5 \mathrm{atm} \mathrm{to} 0.25 \mathrm{atm} \mathrm{is} 10 \text{seconds, then , calculate the order of the reaction?}$

Concentration of reactant $\mathrm{A}$ is plotted against time $\text{'}\mathrm{t}\text{'}$for the reactions of different order. Which of the following plot is/are correct ?

In the reaction, $\mathrm{P}+\mathrm{Q}\to \mathrm{R}+\mathrm{S}$ the time taken for $75\%$the reaction of $\mathrm{P}$ is twice the time taken for $50\%$ reaction of $\mathrm{P}$. The concentration of $\mathrm{Q}$ varies with reaction time as shown in the figure. The overall order of the reaction is: