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

Decomposition of $\mathrm{HI}\left(\mathrm{g}\right)$ on Gold surface is zero order reaction. Initially few moles of ${\mathrm{H}}_2$ are present in container then which of the following graph is correct?

For a reaction $\mathrm{A}\stackrel{{\mathrm{k}}_{\mathrm{r}}=0.6\mathrm{M} {\min }^{-1}}{\to }2\mathrm{B}$ starting with $1\mathrm{M}$ of $\mathrm{A}$ only. Then calculate the concentration of $\mathrm{B}\left(\mathrm{in} \mathrm{M}\right)$ after $100 \sec \mathrm{and} 200 \sec$respectively are

For the reaction $A+B\to$ products, the following initial rates were obtained at various given initial concentrations. Determine the half-life period.

$\begin{array}{|cccc|}\hline \mathrm{S}.\mathrm{No}. & [\mathrm{A} ]{\mathrm{molL}}^{-1}& \left[\mathrm{B}\right] {\mathrm{molL}}^{-1}& \mathrm{Initial}\mathrm{rate} {\mathrm{Ms}}^{-1} \\ 1. & 0.1& 0.1& 0.05\\ 2.& 0.2& 0.1& 0.10\\ 3.& 0.1& 0.2& 0.05\\ \hline\end{array}$

Select the correct statements out of I, II and III for a zero order reaction:

I. Quantity of the product formed is directly proportional to time.

III. If $50\%$ reaction takes place in $100$ minutes, $75\%$ reaction will take place in $150$ minutes.

III.Larger the initial concentration of the reactant, greater is the half-life period.

In a reaction, the initial concentration of the reactants increases fourfold and the rate becomes eight times its initial value. The order of the reaction is -

The half-life of a radioisotope is $6.93$ hours. If initial mass of the isotope is $200 \mathrm{g}$, the mass (in $\mathrm{g}$) of the remaining undecayed isotope after $46.06$ hours is

The rate-constant of a reaction is $3.5\times {10}^{-12}{\mathrm{s}}^{-1}$. The half-life of this reaction (in s) is

Select the correct statement for a first-order reaction from the following.

The rate constant for the first-order reaction is $60\mathrm{ }{\mathrm{s}}^{-1}$. How much time will it take to reduce the concentration of the reactant to $1/16$ of initial value?

If 50 % of a reaction occurs in 100 second and 75 % of the reaction occurs in 200 second, the order of this reaction is:

Which of the following curve represent zero order reaction of $\mathrm{A}\mathrm{ }\to \mathrm{ }$products?

The inactivation of a viral preparation in a chemical bath is found to be a first order reaction. Calculate the rate constant for the viral inactivation if in the beginning $1.5\mathrm{ }\mathrm{\%}$ of the virus is inactivated per minute.

 $\left(\mathrm{Given}:\ln \frac{100}{98.5}=0.01511\right)$

Two first-order reactions have half times in the ratio of $8 : 1.$ The ratio of time intervals ${\mathrm{t}}_1:{\mathrm{t}}_2$ is:

Here, the time ${\mathrm{t}}_1$ and ${\mathrm{t}}_2$ are time period for ${\left(\frac{1}{4}\right)}^{\mathrm{th}}$ and ${\left(\frac{3}{4}\right)}^{\mathrm{th}}$ completion.

Which of the following equations represent integrated rate equation of zero order reaction?

Which of the following is incorrect?

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

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: