Integrated Rate Law for Zero and First Order Reactions

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

For a zero-order reaction, with the initial reactant concentration $\mathrm{a}$, the time for completion of the reaction is:

Which of the following is incorrect?

The accompanying figure depicts the change in concentration of species $\mathrm{X}$ and $\mathrm{Y}$ for the elementary reaction $\mathrm{X}\to \mathrm{Y}$ as a function of time. The point of intersection of two curves represents:

The order of a reaction for which a linear line (with a negative slope) is obtained in a graph of $\log (\mathrm{a}-\mathrm{x})$ vs $\mathrm{t}$ is:

Two-third life for a first-order reaction is $55$ minutes. The value of its velocity constant is nearly

The time taken for the completion of three-fourths of a first-order reaction is

The half-life period for a zero order reaction is equal to:

 Show that, In a first order reaction, time required for completion of $99.9\%$ is _____ times of half life. ($\log 10 = 1$).

The half-life period of a zero order reaction $\mathrm{A} \to$ product is given by:

A first order reaction has reaction constant, $\mathrm{k}=5.5\times {10}^{-14}{\mathrm{s}}^{-1}$. The half-life of the reaction in seconds is: _____ $\times {10}^{14}$

A reaction occurs by the following mechanism:
(i) ${\mathrm{NO}}_2\left(\mathrm{g}\right)+{\mathrm{F}}_2\left(\mathrm{g}\right)\to {\mathrm{NO}}_2\mathrm{F}\left(\mathrm{g}\right)+\mathrm{F}\left(\mathrm{g}\right)$
(ii) $\mathrm{F}\left(\mathrm{g}\right)+{\mathrm{NO}}_2\left(\mathrm{g}\right)\to {\mathrm{NO}}_2\mathrm{F}\left(\mathrm{g}\right)$
The net reaction is:

The half life of first order reaction is $6.0$ hours. Time  take (in hours) for the concentration of reactant to decrease from $0.8 \mathrm{M}$ to $0.25 \mathrm{M}$ is:

A first order reaction takes $40$ minutes for $20\%$ decomposition. Calculate half life?

Rate constant of a chemical reaction is $1.72\times {10}^{–4} {\mathrm{s}}^{–1}$. Calculate the order of reaction?

What is the mathematical relation between half life of zero order reaction and its rate constant. 

The half-life is the time in which the concentration of the reactant is reduced to half of its initial concentration.

The reaction ${\mathrm{SO}}_2{\mathrm{Cl}}_2 \left(\mathrm{g}\right)\to {\mathrm{SO}}_2 \left(\mathrm{g}\right)+{\mathrm{Cl}}_2 \left(\mathrm{g}\right)$ is a first order gas reaction with $\mathrm{k}=2.2\times {10}^{-5}{\sec }^{-1}$. What percentage of ${\mathrm{SO}}_2{\mathrm{Cl}}_2$ is decomposed on heating this gas for $90 \min$?

For next two question please follow the same

In a vessel gaseous dimethyl ether at initial pressure 'p₀' atm. Dimethyl ether decomposes on heating as per the reaction by first order kinetics.

${\text{CH}}_3-\text{O}-{\text{CH}}_3\left(\text{g}\right)\stackrel{\Delta }{\to }{\text{CH}}_4\left(\text{g}\right)+\text{CO}\left(\text{g}\right)+{\text{H}}_2\left(\text{g}\right)$

It is observed that the half-life period for this reaction is 0.2 h. After a very long time, pressure in the vessel is observed to be 1.2 atm. Assume ideal behaviour of all gases with constant V-T conditions.

What would be the approximate pressure in the vessel at 0.6 h ? $\left[{\text{log}}_{8}8\approx \text{0.9}\right]$