Chemical Kinetics

In a reaction,$2\text{N}_2\text{O}_{5(g)} \rightarrow 4\,\text{NO}_{2(g)} + \text{O}_{2(g)}$$\text{N}_2\text{O}_5$ disappears at a rate of $0.06$ mol dm$^{-3}$ s$^{-1}$Calculate rate of formation of $\text{O}_{2(g)}$ ?

Calculate rate constant of a first order reaction having half life $1$ minute $40$ second?

Identify correct statement regarding order of reaction from following.

What is the order and molecularity of the following elementary reaction?$2\text{NO}_{2(g)} \rightarrow 2\text{NO}_{(g)} + \text{O}_{2(g)}$, rate $= k \times [\text{NO}_2]^2$

Calculate the rate constant of first order reaction $\text{A} \rightarrow \text{B}$ having rate $5.4 \times 10^{-6}\ \text{mol dm}^{-3}\text{s}^{-1}$ and $[\text{A}] = 0.3$ M.

What is the role of catalyst in reaction?

Rate constant of decomposition of hydrogen peroxide is $0.0204\ \text{minutes}^{-1}$, calculate half life of reaction.

A first order reaction take $30$ minutes for $75\%$ decomposition, calculate its rate constant ?

Which of the following is an elementary reaction ?

For a first order reaction, half life is $5$ hour. What time is required to reduce $10$ g of reactant to $2.5$ g ?

Consider the reaction,$3\text{I}^-_{(aq)} + \text{S}_2\text{O}_8^{2-}{}_{(aq)} \longrightarrow \text{I}_3^-{}_{(aq)} + 2\text{SO}_4^{2-}{}_{(aq)}$If the rate of formation of $\text{SO}_4^{2-}$ at a particular time is $2.2 \times 10^{-2}\,\t...

Half life of a first order reaction is $900$ second. If initial concentration of reactant is $0.08\,\text{mol dm}^{-3}$ find concentration that remains after $35$ minute ?

Which of the following reactions has of overall order $1.5$ ?

For the reaction $2\text{NOBr}_{(g)} \longrightarrow 2\text{NO}_{(g)} + \text{Br}_{2(g)}$, rate law is $r = k[\text{NOBr}]^2$. Rate constant is $1.62\ \text{M s}^{-1}$ and concentration of NOBr is $5 \times 10^{-3}\ \text{M}$,What is rate o...

In a first order reaction 20 millimole of reactant is lowered to 10 millimole in $0.3010$ minute. Find rate constant of the reaction?

For a reaction $\text{A} \longrightarrow$ product, $k = 2 \times 10^{-2}\ \text{s}^{-1}$. If the initial concentration of A is $1.0\ \text{mol dm}^{-3}$ find the value of $\log \dfrac{1}{[A]_t}$ after 100 second ?

What is the time required for 75 % completion of a first order reaction if rate constant is $23.03\ \text{minute}^{-1}$ ?

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

If time required for 90 % completion of a first order reaction is '$t$'. What is the time required for 99.9 % completion of reaction at same temperature?

What is the term used for the minimum kinetic energy required for the reactant molecules to undergo reaction?

Half life of zero order reaction is 1 hour. If initial concentration of reactant is 2.0 mol $\text{L}^{-1}$, find the time required to decrease concentration from 0.50 to 0.25 mol $\text{L}^{-1}$

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

In first order reaction 20 millimole of reactant is reduced to 10 millimole in $1 \cdot 151$ minute. Find rate constant.

For the reaction $2\text{NOBr}_{(g)} \rightarrow 2\text{NO}_{(g)} + \text{Br}_{2(g)}$ rate law is $r = k[\text{NOBr}]^2$, if rate constant is $1 \cdot 62 \text{ mol dm}^{-3}\text{ s}^{-1}$ and concentration of NOBr is $2 \times 10^{-3} \tex...

The rate constant for the reaction $2\text{N}_2\text{O}_5 \rightarrow 4\text{NO}_2 + \text{O}_2$ is $3.0 \times 10^{-5}\ \text{s}^{-1}$. If the rate is $2.4 \times 10^{-5}\ \text{mole L}^{-1}\ \text{s}^{-1}$ then the concentration of $\text...

The rate constant of reaction is $1.5 \times 10^7\ \text{s}^{-1}$ at 300 K and $3.0 \times 10^7\ \text{s}^{-1}$ at 330 K. What is the activation energy for the reaction? [ $R \times 2.303 = 19.15\ \text{JK}^{-1}\text{mol}^{-1}$]

The equation for the rate constant is $k = Ae^{-E_a/RT}$.A chemical reaction will proceed more rapidly if there is a decrease in

If for a first-order reaction, $[A]_0 = 1.0\ \text{M}$ and $[A]_t = 0.25\ \text{M}$ after 276 s, find the value of the rate constant (k).

The rate law for the reaction $A + B \rightarrow P$ is found to be rate $= k[A]^2[B]$.The rate constant of the reaction at 300 K is $6.0\ \text{M}^{-2}\text{s}^{-1}$. Calculate the rate of the reaction when $[A] = 1\ \text{M}$ and $[B] = 0....

What is the value of the slope of a graph obtained by plotting the concentration of reactant $(A)_t$ versus time for zero order reaction?

The rate of the reaction $2A + 3B \rightarrow 2C + D$ is $6 \times 10^{-4} \text{ mol dm}^{-3}\text{ s}^{-1}$, when $[A] = [B] = 0.3 \text{ mol dm}^{-3}$. If the reaction is of first order for A and zeroth order for B, then find the rate co...

The time required for $90\%$ completion of a certain first order reaction is $1$ hour. Calculate the time required for $99.9\%$ completion of the same reaction.

What is the role of catalyst in catalytic reaction ?

For the reaction $2\text{A} \longrightarrow 3\text{C} + \text{D}$, the rate of reaction is represented by

The rate of reaction $\text{A} + \text{B} \rightarrow \text{P}$ is $4 \times 10^{-2}\ \text{mol dm}^{-3}\ \text{s}^{-1}$When $[A] = 0.2\ \text{mole dm}^{-3}$ and $[B] = 0.1\ \text{mole dm}^{-3}$, What is the rate constant of reaction, if it...

Identify a type of order of reaction that its unit of rate constant is mol dm$^{-3}$s$^{-1}$ from the following.

In first order reaction, 20 % concentration remains after 10 min. What would be the rate constant of reaction if $\log_{10}(5) = 0.6989$?

For the reaction, $A + B \rightarrow P$, the rate law is rate $= k[A][B]^2$. The rate of reaction is $0.25 \text{ Ms}^{-1}$ when $[A] = 1$ M, $[B] = 0.2$ M at $25^\circ$C. Calculate the rate constant of the reaction at the same temperature.

The rate constant of a reaction is $k = 3.28 \times 10^{-4}$ s$^{-1}$. Find the order of the reaction.

The half-life of a first-order reaction is $20$ minutes. What is the rate constant (in min$^{-1}$) for this reaction?

A first order reaction takes $16$ minutes for it's $50\%$ completion. What fraction that would react in $32$ minutes from the beginning?

Which of the following statements is NOT true about the rate constant?

The rate constant for a first order reaction is $60 \text{ s}^{-1}$. How much time will it take to reduce the concentration of the reactant to $1/20^{\text{th}}$ of its initial value?

A first order reaction complete $60$% in $20$ minutes. How long will the reaction take to complete $84$%?

What is the order of the following reaction ?$2\text{H}_2\text{O}_2 (l) \rightarrow 2\text{H}_2\text{O} (l) + \text{O}_2 (g)$, if rate = $k [\text{H}_2\text{O}_2]$

Half life period of a first order reaction is $1386$ seconds. The rate constant of the reaction is

The half life of first order reaction is $850$ s. The initial concentration of the reactant is $0.06$ mol $\text{dm}^{-3}$. What concentration would remain after $1200$ s ?

What is half life of a first order reaction if time required to decrease concentration of reactant from 0.4 M to 0.1 M is $x$ hour?

For the reaction,
\(2 \mathrm{~N}_2 \mathrm{O}_{5(\mathrm{~g})} \longrightarrow 4 \mathrm{NO}_{2(\mathrm{~g})}+\mathrm{O}_{2(\mathrm{~g})}\)
$\mathrm{N}_2 \mathrm{O}_5$ disappears at a rate of $x \mathrm{~mol} \mathrm{dm}^{-3} \mathrm{~s}...

Which of the following statements is NOT correct regarding order of reaction?