Rate of a Chemical Reaction

In a pseudo first order hydrolysis of ester in water, the following results are obtained:

(i) The average rate of reaction between the time interval 30 to 60 seconds and

(ii) The pseudo first order rate constant for the hydrolysis of ester is?

Consider a reaction $a\text{G}+\text{bH}\to \text{products}$.  When concentration of both the reactants $\mathrm{G}$ and $\mathrm{H}$ is doubled, the rate increases by eight times. However, when the concentration of $\mathrm{G}$ is doubled, keeping the concentration of $\mathrm{H}$ constant, the rate is doubled. The overall order of the reaction is:

Consider the chemical reaction:

${\text{N}}_2\left(\text{g}\right)+3{\text{H}}_2\left(\text{g}\right)⟶2{\text{NH}}_3\left(\text{g}\right)$

The rate of this reaction can be expressed in terms of time derivatives of concentration of  $N_2\left(\text{g}\right)\text{ , }{\text{H}}_2\left(\text{g}\right)\text{ and }{\text{NH}}_3\left(\text{g}\right)$ Identify the correct relationship amongst the rate expressions:

For a certain reaction, the rate $=\mathrm{k} [\mathrm{A}{]}^2 [\mathrm{B}]$, when the initial concentration of A is tripled keeping concentration of B constant, the initial rate would 

${\mathrm{KClO}}_3 + 6{\mathrm{FeSO}}_4 + 3{\mathrm{H}}_2{\mathrm{SO}}_4 \to \mathrm{KCl} + 3{\mathrm{Fe}}_2({\mathrm{SO}}_4{)}_3 + 3{\mathrm{H}}_2\mathrm{O}$

The above reaction was studied at $300 \mathrm{K}$ by monitoring the concentration of ${\mathrm{FeSO}}_4$ in which initial concentration was $10 \mathrm{M}$ and after half an hour became $8.8 \mathrm{M}$. The rate of production of ${\mathrm{Fe}}_2({\mathrm{SO}}_4{)}_3$ is _______ $\times \mathrm{l}{0}^{–6} \mathrm{mol} {\mathrm{L}}^{–1} \mathrm{s}{ }^{–1}$

(Nearest integer)

In the first order decomposition of $\mathrm{A}$:

$\mathrm{A}\stackrel{}{\to }2\mathrm{B}+3\mathrm{C}$

Concentration of $\mathrm{A}$ decreases from $0.8 \mathrm{M} \mathrm{to} 0.2 \mathrm{M}$ in $13.86 \min$. The rate of appearance of $\mathrm{B}\left(\mathrm{in} \mathrm{M}/\mathrm{s}\right)$ after $13.86 \min$ is $\mathrm{y}\times {10}^{-2}\mathrm{M} {\min }^{-1}$. The value of $\mathrm{y}$ is(The nearest integer)

The reaction, $2{\mathrm{NO}}_{\left(\mathrm{g}\right)}+{{\mathrm{Cl}}_2}_{\left(\mathrm{g}\right)}\stackrel{}{\to }2{\mathrm{NOCl}}_{\left(\mathrm{g}\right)}$ is carried out in a closed vessel. if partial pressure of $\mathrm{NO}$ is decreasing at the rate of $180 \mathrm{torr}/\min$. what is the rate of change of total pressue of vessel (in torr/min)

In the process ${\mathrm{nA}}_{\left(\mathrm{g}\right)}\to {\mathrm{mB}}_{\left(\mathrm{g}\right)}$ rate of disappearance of A is $5 \times {10}^{-3}\mathrm{M} {\min }^{-1}$ & rate of appearance of B is ${10}^{-2} \mathrm{M} {\min }^{-1}$ at same instant. Then values of n & m respectively are

For a reaction $2\mathrm{A} + \mathrm{B} \to 3\mathrm{Z}$, if the rate of consumption of A is $2 \times {10}^{-4} \mathrm{mol} {\mathrm{dm}}^{-3}{\mathrm{s}}^{-1}$ , the rate of formation of Z will be

For a reaction $\mathrm{A}+\mathrm{B}\to$ products, the rate of reaction was doubled when the concentration of $\mathrm{A}$ was doubled. When concentration of $\mathrm{A}$ and $\mathrm{B}$ both was doubled, the rate was again doubled, order of reaction with respect to $\mathrm{A}$ and $\mathrm{B}$ are

$\mathrm{A}\underset{{\mathrm{k}}_2}{\overset{{\mathrm{k}}_1}{\rightleftharpoons }}\mathrm{B}$

Select the correct option for net rate of $\mathrm{A}$

Hydrogen gas, ${\mathrm{H}}_2\left(\mathrm{g}\right)$, reacts with iodine gas, ${\mathrm{I}}_2\left(\mathrm{g}\right)$, to form hydrogen iodide, $\mathrm{HI}\left(\mathrm{g}\right)$:

${\mathrm{H}}_2\left(\mathrm{g}\right) + {\mathrm{I}}_2\left(\mathrm{g}\right) \to 2\mathrm{HI}\left(\mathrm{g}\right)$

The mechanism of the two-step reaction is considered to be:

step $1$: ${\mathrm{I}}_2\left(\mathrm{g}\right) \underset{{\mathrm{k}}_{-1}}{\overset{{\mathrm{k}}_1}{\leftrightharpoons }} 2\mathrm{I}\left(\mathrm{g}\right)$                        fast

step $2$: $2\mathrm{I}\left(\mathrm{g}\right) + {\mathrm{H}}_2\left(\mathrm{g}\right) \stackrel{{\mathrm{k}}_2}{\to } 2\mathrm{HI}\left(\mathrm{g}\right)$     slow

What is the rate equation for the overall reaction?

Select the correct expressions about the rate of appearance of the product is related to the disappearance of the reactant.

${\mathrm{BrO}}_3^{-} \left(\mathrm{aq}\right)+5{\mathrm{Br}}^{-} \left(\mathrm{aq}\right)+6{\mathrm{H}}^{+} \left(\mathrm{aq}\right)⟶3{\mathrm{Br}}_2 \left(\mathrm{l}\right)+3{\mathrm{H}}_2\mathrm{O} \left(\mathrm{l}\right)$

For the non-equilibrium process: $\mathrm{A}+\mathrm{B}\to \mathrm{P}$, the reaction is of the first order with respect to $\mathrm{A}$ and of the second order with respect to $\mathrm{B}$. If $1$ mole each of $\mathrm{A}$ and $\mathrm{B}$ are introduced into a $1 \mathrm{litre}$ flask, and the initial rates were $1\times {10}^{-2} \mathrm{mol}/\mathrm{L},$ calculate the rate when half the reactants have converted to the product.

If the answer is of type $\mathrm{y}\times {10}^{-5} \mathrm{M} {\sec }^{-1}$, report the value of $\mathrm{y}$.

Find the value of the rate constant for the reaction: $\mathrm{A}+\mathrm{B}\to \mathrm{AB},$ if the rate of the reaction is $5\times {10}^{-5} (\mathrm{mol} {\mathrm{L}}^{-1}){\min }^{-1}$ and $\left[\mathrm{A}\right]$ and $\left[\mathrm{B}\right]$ are respectively, $0.05$ and $0.01 \mathrm{mol} {\mathrm{L}}^{-1}$.

Give answer after multiplying with 10.

For a given reaction $3\mathrm{A}\mathrm{ }+\mathrm{B}\to \mathrm{C}+\mathrm{D}$ the rate of reaction can be represented by

The term $\frac{-\mathrm{dc}}{\mathrm{dt}}$ in a rate equation refers to: