Dependence of Rate on Reactant Concentrations

In a first-order reaction, the concentration of reactant decreases from $\text{800}{\text{ mol/dm }}^3{\text{ to 50 mol/dm }}^3$ in$2 \times {10}^2 \mathrm{s}$. The rate constant of reaction in ${\mathrm{s}}^{-1}$ is

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

What is meant by specific reaction rate?

Give the general expression for a balanced chemical equation by applying the law of mass action.

What is the order of a reaction whose rate constant is $5 \mathrm{x} {10}^{-4} {\mathrm{mol}}^{-1}\mathrm{litre} {\mathrm{s}}^{-1}$?

At $30°\mathrm{C}$, the half life for the decomposition of ${\mathrm{AB}}_2$ is $200 \mathrm{s}$ and is independent of the initial concentration of ${\mathrm{AB}}_2$. The time required for $80\%$ of the ${\mathrm{AB}}_2$ to decompose is (Given: $\log 2 = 0.30; \log 3 = 0.48$)

The unit of rate constant of a reaction is $\mathrm{mole} {\mathrm{litre}}^{-1} {\mathrm{second}}^{-1}$. What is its order? Write the rate equation of the following reaction 

$2{\mathrm{NO}}_2\to {\mathrm{N}}_2{\mathrm{O}}_4$

$\mathrm{A}\to \mathrm{B}+\mathrm{C}$

The rate constant of the given reaction is $2.5\times {10}^2$ $\mathrm{mole} {\mathrm{lit}}^{-1} {\sec }^{-1}$ at initial concentration of reactant $0.5\mathrm{M}$. Calculate order of reaction.

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 

The number of incorrect statement/s from the following is ______________

A. The successive half lives of zero order reactions decreases with time.

B. A substance appearing as reactant in the chemical equation may not affect the rate of reaction

C. Order and molecularity of a chemical reaction can be a fractional number

D. The rate constant units of zero and second order reaction are $\mathrm{molL}{}^{-1} {\mathrm{s}}^{-1}$ and ${\mathrm{mol}}^{-1} \mathrm{L} {\mathrm{s}}^{-1}$ respectively

In an enzyme solution, sucrose undergoes fermentation. If $0.10 \mathrm{mol}/\mathrm{L}$ solution of sucrose is reduced to $0.05 \mathrm{mol}/\mathrm{L}$ in $10$ hours and to $0.025 \mathrm{mol}/\mathrm{L}$ in $20$ hours, then the rate constant of the reaction will be?

${\mathrm{t}}_{87.5}$ is the time required for the reaction to undergo $87.5\%$ completion and ${\mathrm{t}}_{50}$ is the time required for the reaction to undergo $50\%$ completion. The relation between ${\mathrm{t}}_{87.5}$ and ${\mathrm{t}}_{50}$ for a first order reaction is ${\mathrm{t}}_{87.5}=\mathrm{x}\times {\mathrm{t}}_{50}$
The value of $\mathrm{x}$ is $\_\_\_\_\_\_\_\_\_.$ (Nearest integer)

$\mathrm{A}\left(\mathrm{g}\right)\to 2 \mathrm{B}( \mathrm{g})+\mathrm{C}\left(\mathrm{g}\right)$ is a first order reaction. The initial pressure of the system was found to be $800 \mathrm{mm} \mathrm{Hg}$ which increased to $1600 \mathrm{mm} \mathrm{Hg}$ after $10 \min$. The total pressure of the system after $30$min will be $\mathrm{mm} \mathrm{Hg}$. (Nearest integer)

A molecule undergoes two independent first order reactions whose respective half lives are $12 \min$ and $3 \min$. If both the reactions are occurring then the time taken for the $50\%$ consumption of the reactant is ______ $\min$. (Nearest integer)