Chemical Kinetics

Calculate the rate constant of the first order reaction if \(80 \%\) of the reactant decomposes in 60 minutes.

Which from following is the slope of the graph of \([\mathrm{A}]_{\mathrm{t}}\) versus time for zero order reaction?

Calculate the rate constant of the first order reaction if \(20 \%\) of the reactant decomposes in 15 minutes.

Find the rate of formation of \(\mathrm{NO}_{2(\mathrm{~g})}\) in the following reaction.
$$\begin{aligned}
& 2 \mathrm{~N}_2 \mathrm{O}_{5(\mathrm{~g})} \rightarrow 4 \mathrm{NO}_{2(\mathrm{~g})}+\mathrm{O}_{2(\mathrm{~g})} \\
& {\left[\fr...

For the reaction, \(2 A+2 B \longrightarrow 2 C+D\), the rate law is expressed as rate \(=k[A]^2[B]\).
Calculate the rate constant if rate of reaction is \(0.24 \mathrm{~mol} \mathrm{~dm}^{-3} \mathrm{~s}^{-1}\).
[[\(A\)]\(=0.5 \mathrm{M}\)...

For the reaction,
\(\mathrm{CH}_3 \mathrm{Br}(a q)+\mathrm{OH}^{-}(a q) \longrightarrow \mathrm{CH}_3 \mathrm{OH}(a q)+\mathrm{Br}^{-}(a q),\)
The rate law is rate \(=k\left[\mathrm{CH}_3 \mathrm{Br}\right]\left[\mathrm{OH}^{-}\right]\). W...

Which from following statements about rate constant is NOT true?

Identify rate law expression for \(2 \mathrm{NO}_{(\mathrm{g})}+\mathrm{Cl}_{2(\mathrm{~g})} \rightarrow 2 \mathrm{NOCl}_{(\mathrm{g})}\) if the reaction is second order in \(\mathrm{NO}\) and first order in \(\mathrm{Cl}_2\).

Calculate the rate constant of first order reaction if half life of reaction is 40 minutes.

Calculate the time needed for reactant to decompose \(99.9 \%\) if rate constant of first order reaction is 0.576 minute\(^{-1}\).

The rate law for the reaction \(\mathrm{A}+\mathrm{B} \rightarrow \mathrm{C}\) at \(25^{\circ} \mathrm{C}\) is given by rate \(=k[A][B]^2\). Calculate the rate of reaction if rate constant at same temperature is $$6.25 \mathrm{~mol}^{-2} \m...

A first order reaction takes 23.03 minutes for \(20 \%\) decomposition. Calculate its rate constant.

What is half life time of a first order reaction if initial conc. of reactant is \(0.01 \mathrm{~mol} \mathrm{~L}^{-1}\) and rate of reaction is \(0.00352 \mathrm{~mol} \mathrm{~L}^{-1}\) minute \(^{-1}\) ?

Slope of the graph between \(\log \frac{[\mathrm{A}]_0}{[\mathrm{~A}]_{\mathrm{t}}}\) (y axis) and time ( \(x\) axis) for first order reaction is equal to:

For an elementary reaction
\(2 \mathrm{~A}+\mathrm{B} \longrightarrow 3 \mathrm{C}\)
rate of appearance of \(\mathrm{C}\) is \(1.3 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}\), the rate of disappearance of \(\mathrm{A}\)...

Identify the expression for average rate for following reaction.
\(\mathrm{N}_{2(\mathrm{~g})}+3 \mathrm{H}_{2(\mathrm{~g})} \rightarrow 2 \mathrm{NH}_{3(\mathrm{~g})}\)

Calculate the rate constant of the first order reaction if \(80 \%\) of the reactant reacted in 15 minute.

For a reaction \(\mathrm{A}+\mathrm{B} \rightarrow\) product, if \([\mathrm{A}]\) is doubled keeping \([\mathrm{B}]\) constant, the rate of reaction doubles. Calculate the order of reaction with respect to A.

The reaction, \(3 \mathrm{ClO}^{-} \rightarrow \mathrm{ClO}_3^{-}+2 \mathrm{Cl}^{-}\) occurs in two steps:
i. \(\quad 2 \mathrm{ClO}^{-} \rightarrow \mathrm{ClO}_2^{-}+\mathrm{Cl}^{-}\)
ii. $$\quad \mathrm{ClO}_2^{-}+\mathrm{ClO}^{-} \right...

What is the half life of a first order reaction if rate constant is \(4.2 \times 10^{-2}\) per day?

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

Time required for \(90 \%\) completion of a first order reaction is '\(x\)' minute. Calculate the time required to complete \(99.9 \%\) of the reaction at same temperature.

Calculate the rate constant for the first order reaction, \(\mathrm{A} \rightarrow \mathrm{B}\) if the rate of reaction is \(5.4 \times 10^{-6} \mathrm{~mol} \mathrm{~dm}^{-3} \mathrm{~s}^{-1}\) and \([\mathrm{A}]=0.3 \mathrm{M}\).

Find the average rate of formation of \(\mathrm{NO}_{2(\mathrm{~g})}\), in following reaction.
$$\begin{aligned}
& 2 \mathrm{~N}_2 \mathrm{O}_{5(\mathrm{~g})} \rightarrow 4 \mathrm{NO}_{2(\mathrm{~g})}+\mathrm{O}_{2(\mathrm{~g})} \\
& {\lef...

If rate of reaction is given as
\(\frac{1}{3} \frac{\mathrm{d}[\mathrm{x}]}{\mathrm{dt}}=-\frac{1}{2} \frac{\mathrm{d}[\mathrm{y}]}{\mathrm{dt}}=-\frac{\mathrm{d}[\mathrm{Z}]}{\mathrm{dt}}\),
the reaction can be represented as

Find the rate constant of first order reaction in second having half life of 2.5 hours.

For the reaction \(\mathrm{N}_{2(\mathrm{~g})}+3 \mathrm{H}_{2(\mathrm{~g})} \rightarrow 2 \mathrm{NH}_{3(\mathrm{~g})}\), rate of disappearance of \(\mathrm{N}_{2(\mathrm{~g})}\) is \(2.22 \times 10^{-3} \mathrm{~mol} \mathrm{~dm}^{-3}\). ...

A reaction is first order with respective to \(\mathrm{A}\) and second order with respective to \(\mathrm{B}\). What is the effect on reaction rate if concentration of B is increased 3 times?

If decomposition of hydrogen peroxide is a first order reaction, it's rate law equation can be represented as

For the reaction \(\mathrm{A}+\mathrm{B} \rightarrow\) product, rate of reaction is \(3.6 \times 10^{-2} \mathrm{mol~dm}^{-3} \mathrm{sec}^{-1}\). When \([\mathrm{A}]=0.2 \mathrm{~mol} \mathrm{dm}^{-3}\) and $$[\mathrm{B}]=0.1 \mathrm{~mol}...

In a first reaction 60% of reactant decomposes in 4.606 min. What is half life of reaction? (k = 0.1989 min\(^{-1}\))

Half-life and rate constant for first order reaction are related by equation,

For the reaction, \(2 \mathrm{~A}+\mathrm{B} \rightarrow 2 \mathrm{C}\), rate of disappearance of \(\mathrm{A}\) is \(0.076 \mathrm{~mol} \mathrm{~s}^{-1}\). What is the rate of disappearance of \(\mathrm{B}\) ?

The order of reaction for which the units of rate constant are \(\mathrm{mol} \mathrm{~dm}^{-3} \mathrm{~s}^{-1}\) is

Time required for \(90 \%\) completion of a first order reaction is \(t\). What is the time required for completion of \(99 \%\) reaction?

The rate law equation for a reaction between \(\mathrm{A}, \mathrm{B}\) and \(\mathrm{C}\) is \(\mathrm{r}=\mathrm{k}[\mathrm{A}][\mathrm{B}][\mathrm{C}]^2\), what will be ne rate of reaction if concentration of both \(\mathrm{A}\) and $$\m...

Which of the following equations represents integrated rate law for zero order reaction?

Ammonia and oxygen react at high temperature as
\(4 \mathrm{NH}_{3(\mathrm{~g})}+5 \mathrm{O}_{2(\mathrm{~g})} \longrightarrow 4 \mathrm{NO}_{(\mathrm{g})}+6 \mathrm{H}_2 \mathrm{O}_{(\mathrm{g})} \text {. }\)
If rate of formation of $$\mat...

Which of the following represents integrated rate law equation for gas phase first order reaction, \(\mathrm{A}_{(\mathrm{g})} \rightarrow \mathrm{B}_{(\mathrm{g})}+\mathrm{C}_{(\mathrm{g})}\)
if \(\mathrm{P}_{\mathrm{i}}=\) initial pressur...

For the reaction \(2 \mathrm{~A}+2 \mathrm{~B} \rightarrow 2 \mathrm{C}+\mathrm{D}\) if \(\mathrm{r}=\mathrm{k}[\mathrm{A}]^2[\mathrm{~B}]^0\), then rate of reaction is

Identify order of reaction if it's rate constant is x sec\(^{-1}\).

For a reaction \(\mathrm{A} \rightarrow\) product, rate constant is \(2 \times 10^{-2} \mathrm{~s}^{-1}\). The initial concentration of \(\mathrm{A}\) is 1.0 mol dm\({ }^{-3}\). What is the value of $$\log \frac{1}{[\mathrm{~A}]_{\mathrm{t}...

Which of the following statements is NOT true for a reaction having rate law \(\mathrm{r}=\mathrm{k}\left[\mathrm{H}_2\right]\left[\mathrm{I}_2\right]\) ?

What is rate constant of a first order reaction if 0.08 mole of reactant reduces to 0.02 mole in 23.03 minute?

For the reaction \(\mathrm{N}_{2(\mathrm{~g})}+3 \mathrm{H}_{2(\mathrm{~g})} \rightarrow 2 \mathrm{NH}_{3(\mathrm{~g})}\),
what is the relation between \(\frac{\mathrm{d}\left[\mathrm{N}_2\right]}{\mathrm{dt}}\) and $$\frac{\mathrm{d}\left[...

In a first order reaction, concentration of reactant is reduced to (1/8)th of concentration in 23.03 minutes. What is half-life period of reaction?

Slope of the graph between rate ( \(\mathrm{Y}\)-axis) and \([\mathrm{A}](\mathrm{X}\)-axis) for the first order reaction is equal to

What is the rate of appearance of \(\mathrm{Z}\) in following reaction? \(3 \mathrm{x} \rightarrow 2 \mathrm{y}+\mathrm{z}\), if rate of disappearance of \(\mathrm{x}\) is \(0.072 \mathrm{~mol} \mathrm{~s}^{-1}\)

What is the rate of disappearance of B in following reaction? \(2 \mathrm{A}+\mathrm{B} \rightarrow 3 \mathrm{C}\), if rate of appearance of \(\mathrm{C}\) is \(1.3 \times 10^{-4} \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}\).

What is the half-life of a first order reaction if time required to decrease concentration of reactant from 1.0 M to 0.25 M is 10 hour?