Chemical Kinetics

Calculate rate constant of a first order reaction having pre exponential factor $1.6 \times 10^{13} \mathrm{~s}^{-1}$.
\(\left(\mathrm{E}_{\mathrm{a}} / 2.303 \mathrm{RT}=21\right)\)

Rate of the reaction $\mathrm{A}+\mathrm{B} \longrightarrow$ product is $3.6 \times 10^{-2} \mathrm{~mol} \mathrm{dm}^{-3} \mathrm{~s}^{-1}$ and rate law is $\mathrm{r}=\mathrm{k}[\mathrm{A}][\mathrm{B}]^2$. What is rate constant of the rea...

Identify the order of following reaction?
\(2 \mathrm{NO}_{2(\mathrm{~g})} \rightarrow 2 \mathrm{NO}_{(\mathrm{g})}+\mathrm{O}_{2(\mathrm{~g})}\)

The slope of a graph $\log [A]_1$ versus ' $t$ ' for first order reaction is $-2.5 \times 10^{-3} \mathrm{~s}^{-1}$. Find rate constant of the reaction?

A complex reaction takes place in following steps.
$$ \begin{aligned} & \mathrm{NO}_2 \mathrm{Cl}_{(\mathrm{g})} \longrightarrow \mathrm{NO}_{2(\mathrm{~g})}+\mathrm{Cl}_{(\mathrm{g})} \text { (slow) } \\ & \mathrm{NO}_2 \mathrm{Cl}_{(\math...

Identify role of glycerol in following reaction.
\(2 \mathrm{H}_2 \mathrm{O}_{2(\ell)} \xrightarrow{\text { glycerol }} 2 \mathrm{H}_2 \mathrm{O}_{(\ell)}+\mathrm{O}_{2(g)}\)

What is the average rate of reaction when change in concentration of product is 0.05 M in 20 seconds?

The rate constant is doubled when temperature increases from $27^{\circ} \mathrm{C}$ to $37^{\circ} \mathrm{C}$. What is activation energy in kJ ?

If $r=k[A]^2[B]$ is rate law equation for reaction $\mathrm{A}+\mathrm{B} \rightarrow \mathrm{C}$, at $[\mathrm{A}]=1 \mathrm{M}$ and $[\mathrm{B}]=0.2 \mathrm{M}$, Calculate rate of reaction if rate constant is $6.25 \mathrm{M}^{-2} \mathr...

For a reaction $\mathrm{A} \rightarrow$ Product, rate constant is $6.93 \times 10^{-3}$ hour ${ }^{-1}$. What is order of reaction?

What is the time required for $99 \%$ completion of a first order reaction if rate constant is $23.03 \mathrm{~min}^{-1}$ ?

If Instantaneous rate of reaction is stated as $-\frac{1}{2} \frac{\mathrm{~d}[x]}{\mathrm{dt}}=-\frac{\mathrm{d}[\mathrm{y}]}{\mathrm{dt}}=\frac{1}{2} \frac{\mathrm{~d}[\mathrm{z}]}{\mathrm{dt}}$, identify the reaction.

Which of the following is an example of second order reaction?

Which of the following is an example of first order reaction?

The rate constant of a first order reaction is $1.15 \times 10^{-3} \mathrm{~s}^{-1}$. How long will 5 g of reactant take to reduce to 3 g ?

Find the rate of following reaction.
\(2 \mathrm{~N}_2 \mathrm{O}_{5(\mathrm{~g})} \longrightarrow 4 \mathrm{NO}_{2(\mathrm{~g})}+\mathrm{O}_{2(\mathrm{~g})}\)
if concentration of $\mathrm{NO}_2$ increases to $5.2 \times 10^{-3} \mathrm{M...

A first order reaction is $50 \%$ completed in 16 minutes. Find the percentage of reactant reacting in 32 minutes.

Rate law for the reaction,
\(\mathrm{NO}_{2(\mathrm{~g})}+\mathrm{CO}_{(\mathrm{g})} \longrightarrow \mathrm{NO}_{(\mathrm{g})}+\mathrm{CO}_{2(\mathrm{~g})}\)
is as $\mathrm{R}=\mathrm{k}\left[\mathrm{NO}_2\right]^2$. What is the order of...

Rate law for the reaction $\mathrm{aA}+\mathrm{bB} \rightarrow \mathrm{cC}+\mathrm{dD}$ is $r=k[A][B]$, the rate of reaction doubles if

Half life of a first order reaction is 20 minutes. The time taken to reduce the initial concentration of reactant to $(1 / 10)^{\text {th }}$ is _________

Nitric oxide reacts with $\mathrm{H}_2$ according to reaction. $2 \mathrm{NO}_{(\mathrm{g})}+2 \mathrm{H}_{2(\mathrm{~g})} \rightarrow \mathrm{N}_{2(\mathrm{~g})}+2 \mathrm{H}_2 \mathrm{O}_{(\mathrm{g})}$, identify correct relation for disa...

The half life values for two different first order reaction A and B are 75 minute and 2.5 hour respectively. What is the $\frac{r_B}{r_A}$ ratio of rate constants?

For a reaction,
$\mathrm{A}+\mathrm{B} \longrightarrow$ product, it is found that rate law is $\mathrm{r}=\mathrm{k}[\mathrm{A}]^{1.5}[\mathrm{~B}]^{2.5}$. What is the order of reaction?

Nitric oxide reacts with $\mathrm{H}_2$ according to reaction. $2 \mathrm{NO}_{(\mathrm{g})}+2 \mathrm{H}_{2(\mathrm{~g})} \rightarrow \mathrm{N}_{2(\mathrm{~g})}+2 \mathrm{H}_2 \mathrm{O}_{(\mathrm{g})}$.
Identify the correct relationship ...

What is the order and molecularity respectively for the elementary reaction given below?
$$ \mathrm{O}_{3(\mathrm{~g})}+\mathrm{O}_{(\mathrm{g})} \longrightarrow 2 \mathrm{O}_{2(\mathrm{~g})} \text { if } \mathrm{r}=\mathrm{k}\left[\mathrm{...

Calculate the time in seconds required to reduce the concentration of reactant to half of initial concentration for first order reaction if rate constant is $1.386 \times 10^{-3} \mathrm{~s}^{-1}$.

Nitric oxide reacts with $\mathrm{H}_2$ according to reaction, $2 \mathrm{NO}_{(\mathrm{g})}+2 \mathrm{H}_{2(\mathrm{~g})} \longrightarrow \mathrm{N}_{2(\mathrm{~g})}+2 \mathrm{H}_2 \mathrm{O}_{(\mathrm{g})}$, identify the correct relations...

Rate law for the reaction $a A+b B \rightarrow c C+d D$ is $\mathrm{r}=\mathrm{k}[\mathrm{A}][\mathrm{B}]$. Which from following conditions does NOT affect the rate of reaction?

For a reaction, $\mathrm{A} \longrightarrow \mathrm{B}$, rate equation is $\mathrm{r}=\mathrm{k}[\mathrm{A}]^{\circ}$. If initial concentration of reactant is 'a'mol dm ${ }^{-3}$ find half life time of reaction.

The rate constant for the reaction, $2 \mathrm{~N}_2 \mathrm{O}_{5(\mathrm{~g})} \rightarrow 2 \mathrm{~N}_2 \mathrm{O}_{4(\mathrm{~g})}+\mathrm{O}_{2(\mathrm{~g})}$ is $4.98 \times 10^{-4} \mathrm{~s}^{-1}$. What is the order of reaction?

Which of the following equations is correct regarding rate of disappearance of reactant and appearance of product for
\(\mathrm{N}_{2(\mathrm{~g})}+3 \mathrm{H}_{2(\mathrm{~g})} \longrightarrow 2 \mathrm{NH}_{3(\mathrm{~g})}\)

The rate constant for a first order reaction is $0.58 \mathrm{~s}^{-1}$ at 300 K and $0.026 \mathrm{~s}^{-1}$ at 290 K .
What is the energy of activation?
\(\left(\mathrm{R}=8.314 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right)\)

If concentration of reactant ' $A$ ' is increased by 10 times, rate of reaction increases 100 times. What is order of reaction if rate law is $r=k[A]^r$ ?

Half life of a first order reaction is 3 minute. What is the time required to reduce the concentration of reactant by $90 \%$ of its initial concentration?

What is order and molecularity of following reaction?
\(\mathrm{NO}_{2(\mathrm{~g})}+\mathrm{NO}_{2(\mathrm{~g})} \longrightarrow 2 \mathrm{NO}_{(\mathrm{g})}+\mathrm{O}_{2(\mathrm{~g})}\)

For the reaction, $\mathrm{NO}_{2(\mathrm{~g})}+\mathrm{CO}_{(\mathrm{g})} \longrightarrow \mathrm{NO}_{(\mathrm{g})}+\mathrm{CO}_{2(\mathrm{~g})}$, rate of formation of $\mathrm{NO}_{(\mathrm{g})}$ is $\mathrm{Y} \mathrm{mol} \mathrm{dm} \...

Which from following is correct regarding $t_{1 / 2}$ of reaction if we double the initial concentration of a reactant in first order reaction?

In a first order reaction concentration of reactant decreases from 20 milli $\mathrm{mol} \mathrm{dm}^{-3}$ to 8 milli $\mathrm{mol} \mathrm{dm}^{-}$ in 40 minutes, find rate constant of reaction?

Rate law for the reaction,
$$ \mathrm{C}_2 \mathrm{H}_5 \mathrm{I}_{(\mathrm{g})} \longrightarrow \mathrm{C}_2 \mathrm{H}_{4(\mathrm{~g})}+\mathrm{HI}_{(\mathrm{g})} \text { is } \mathrm{r}=\mathrm{k}\left[\mathrm{C}_2 \mathrm{H}_5 \mathrm{...

Which from following is a correct representation of reaction rate for reaction stated below?
\(\mathrm{N}_{2(\mathrm{~g})}+3 \mathrm{H}_{2(\mathrm{~g})} \rightleftharpoons 2 \mathrm{NH}_{3(\mathrm{~g})}\)

Half life of a first order reaction is 900 minute at 400 K , find its half life at 300 K ?
\(\left(\frac{\mathrm{E}_{\mathrm{a}}}{2.303 \mathrm{R}}=1.3056 \times 10^3\right)\)

Consider the reaction $3 \mathrm{I}^{-}+\mathrm{S}_2 \mathrm{O}_8^{2-} \longrightarrow \mathrm{I}_3^{-}+2 \mathrm{SO}_4^{2-}$, at a particular time t , $\frac{\mathrm{d}\left[\mathrm{SO}_4^{2-}\right]}{\mathrm{dt}}$ is $2.2 \times 10^{-2} \...

For the reaction, $\mathrm{NO}_{2(\mathrm{~g})}+\mathrm{CO}_{(\mathrm{g})} \longrightarrow \mathrm{NO}_{(\mathrm{g})}+\mathrm{CO}_{2(\mathrm{~g})}$ rate of reaction is proportional to square of $\left[\mathrm{NO}_2\right]$ and independent o...

Find the percentage of unreacted reactant for zero order reaction in 90 second having rate constant $1 \mathrm{~mol} \mathrm{~dm}^{-3} \mathrm{~s}^{-1}$.

The reaction $2 \mathrm{~A}+\mathrm{B}+\mathrm{C} \longrightarrow \mathrm{D}+\mathrm{E}$ is found to be first order in A , second order in B and zero order in C . What is the effect of increasing concentration of all reactants twice?

For the reaction, $\mathrm{N}_{2(\mathrm{g})}+3 \mathrm{H}_{2(\mathrm{g})} \longrightarrow 2 \mathrm{NH}_{3(\mathrm{g})}$
$\mathrm{NH}_3$ is formed at a rate of $0.088 \mathrm{~mol} \mathrm{~dm}^{-3} \mathrm{~s}^{-1}$. Calculate consumption...

Identify order of following reaction.
\(\mathrm{H}_2 \mathrm{O}_{2(\mathrm{~g})} \longrightarrow 2 \mathrm{H}_2 \mathrm{O}_{(\mathrm{l})}+\mathrm{O}_{2(\mathrm{~g})}\)

In the Arrhenius plot of logk versus $1 / T$ find the value of intercept on $y$ axis

Half life of a first order reaction is 1 hour. What fraction of it will remain after 3 hour?

For the reaction,
\(3 \mathrm{I}_{\mathrm{(aq.)}}^{-}+\mathrm{S}_2 \mathrm{O}_{8(\mathrm{aq.})}^{2-} \longrightarrow 2 \mathrm{SO}_{4(\mathrm{aq.})}^{2-}+\mathrm{I}_{3(\mathrm{aq.})}^{-}\)
rate of formation of $\mathrm{SO}_{4(\mathrm{aq.})}...