Order of a reaction

Rate $=\mathrm{K}{\left[\mathrm{A}\right]}^{1/2}{\left[\mathrm{B}\right]}^{3/2}{\left[\mathrm{C}\right]}^{-1}$ order of the 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:

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 :-

The rate of the first order reaction $\mathrm{A}\to$ products is $0.01 \mathrm{M}/\mathrm{s}$, when reactant's concentration is $0.2 \mathrm{M}$. The rate constant for the reaction will be

The slope of the straight line obtained by plotting rate versus concentration of reactant for a first order reaction is.

The unit of rate constant for first order reaction is

Statement $1$: The exponents for concentration do not necessarily match the stoichiometry coefficients in the rate law expression.

Statement $2$: In the rate law expression, exponents for concentration are determined by experiments not by balanced chemical reaction.

$2\mathrm{A}\left(\mathrm{g}\right)\to 3\mathrm{B}\left(\mathrm{g}\right)+2\mathrm{C}\left(\mathrm{g}\right)$ is a first order reaction.

If the initial pressure is $\mathrm{‘}{\mathrm{P}}_0\mathrm{’}$ and the total pressure at time 't' is $\mathrm{‘}{\mathrm{P}}_{\mathrm{t}}\mathrm{’}$, then the rate constant is:

Find out the order for the given reaction


 

Calculate the half life for a zero order reaction, if reaction is $80\%$ completed in $40 \min$.

What is the correct representation of graph for a reaction of first order kinetics (A: moles of reagent remaining, t: time)?

Radioactive decay is an example of which order of reaction? 

Calculate the overall order of the reaction, given that a reaction involving A, B and C as reactants is found to obey the rate law, rate=$\mathrm{k}{\left[\mathrm{A}\right]}^{\mathrm{x}}{\left[\mathrm{B}\right]}^{\mathrm{y}}{\left[\mathrm{C}\right]}^{\mathrm{z}}$. When the concentration of A, B and C are doubled separately, the rate is also found to increase two, zero and four times respectively. 

For a first order reaction, $\mathrm{A}\left(\mathrm{aq}\right)\to \mathrm{B}\left(\mathrm{aq}\right)+\mathrm{C}\left(\mathrm{aq}\right)$ 

$\begin{array}{ccc}\mathrm{Time}& \mathrm{t}& \mathrm{\infty }\\ \mathrm{Moles}\mathrm{ }\mathrm{of}\mathrm{ }\mathrm{reagent}& {\mathrm{n}}_1& {\mathrm{n}}_2\end{array}$

Reaction progress is measure with the help of titration of reagent 'R'. If all $\mathrm{A},\mathrm{ }\mathrm{B}\mathrm{ }\mathrm{and}\mathrm{ }\mathrm{C}$ reacted with reagent and have 'n' factors $\left[\mathrm{n}\mathrm{ }\mathrm{factor};\mathrm{eq}.\mathrm{wt}=\frac{\mathrm{mol}.\mathrm{wt}}{\mathrm{n}}\right]$ in the ratio of 1 : 2 : 3 with the reagent. Calculate k in terms of t, ${\mathrm{n}}_1$ and ${\mathrm{n}}_2$ :

How much time will it take for 99.9% completion if 75% completion of a first order reaction takes 2.38 hours?

The graph which is/are correct for a first-order reaction is:

If ${\mathrm{t}}_{1/2}$ for the reaction is $6.93$ minutes. Then, calculate the time required for the $99.9\%$ completion of a $1^{\text{st }}$ order reaction.

If the time required to complete $96\%$ of reaction $\mathrm{Q}$, which is the same as $50\%$ of reaction $\mathrm{P}$ and the first-order reactions are given below, then find the ratio of the rate constants (${\mathrm{k}}_2/{\mathrm{k}}_1$).

$\mathrm{P}\stackrel{{\mathrm{k}}_1}{⟶}\mathrm{A}+\mathrm{B}$   

$\mathrm{Q}\stackrel{{\mathrm{k}}_2}{⟶}\mathrm{C}+\mathrm{D}$