Consider the following rate expression.

$\mathrm{Rate}=\mathrm{k}{\left[C{H}_{3}CHO\right]}^{\frac{3}{2}}$

The order of reaction and dimension of the rate constant are, respectively-

1. $\raisebox{1ex}{$3$}\!\left/ \!\raisebox{-1ex}{$2$}\right.$; k = ${\mathrm{mol}}^{-1}{\mathrm{Ls}}^{-1}$

2. 3; k = ${\mathrm{mol}}^{-1}{\mathrm{Ls}}^{-1}$

3. $\raisebox{1ex}{$3$}\!\left/ \!\raisebox{-1ex}{$2$}\right.$;  k = ${\mathrm{mol}}^{\frac{1}{2}}{\mathrm{L}}^{-\frac{1}{2}}{\mathrm{s}}^{-1}$

4. $\raisebox{1ex}{$3$}\!\left/ \!\raisebox{-1ex}{$2$}\right.$; k = ${\mathrm{mol}}^{-\frac{1}{2}}{\mathrm{L}}^{\frac{1}{2}}{\mathrm{s}}^{-1}$

What are the dimensions of the rate constant K in the rate law \(\text { Rate }=k\left[H_2 O_2\right]\left[I^{-}\right]\)?
 

For the reaction 2A + B → A₂B, the rate law is rate = k[A][B]², where k = 2.0 × 10⁻⁶ mol⁻² L² s⁻¹,
[A] = 0.1 M, and [B] = 0.2 M. What is the initial rate of the reaction?

1. 0.04$\times {10}^{-9}$ mol ${\mathrm{L}}^{-1}<mspace\; width="1em"></mspace>{\mathrm{s}}^{-1}$

2. 8$\times {10}^{-8}<mspace\; width="1em"></mspace>{\mathrm{mol}}^{-1}\mathrm{L}<mspace\; width="1em"></mspace>{\mathrm{s}}^{-1}$

3. 8$\times {10}^{-9}<mspace\; width="1em"></mspace>\mathrm{mol}<mspace\; width="1em"></mspace>{\mathrm{L}}^{-1}<mspace\; width="1em"></mspace>{\mathrm{s}}^{-1}$

4. 8$\times {10}^{-7}$ mol ${\mathrm{L}}^{-1}<mspace\; width="1em"></mspace>{\mathrm{s}}^{-1}$

The decomposition of NH₃ on a platinum surface is a zero-order reaction. The rates of production of N₂ and H₂ will be respectively:
(given ; k = 2.5 × 10^–4 mol^–1 L s^–1 ) 

The rate equation of a reaction is expressed as, Rate = \(k(P_{CH_{3}OCH_{3}})^{\frac{3}{2}}\)

(Unit of rate = bar min^–1)

The units of the rate constant will be:
1. bar^1/2 min    
2. bar² min^–1   
3. bar^–1 min^–2  
4. bar^–1/2 min^–1

The factor(s) that affect the rate of a chemical reaction is/are:

If the concentration of the reactant is made twice, the new rate of reaction for the second order reaction would be-

1. 2 times

2. 4 times

3. 3 times

4. No change in the rate of the reaction

Which of the following statements regarding the rate constant of a reaction is correct?

$1.$ $6.67$ $\times {10}^{-2}$ $\mathrm{mol}$ ${\mathrm{L}}^{-1}$ ${\mathrm{s}}^{-1}$
$2.$ $2.67$ $\times$ ${10}^{-4}$ $\mathrm{mol}$ ${\mathrm{L}}^{-1}$ ${\mathrm{s}}^{-1}$ $$
$3.$ $4.67$ $\times$ ${10}^{-3}$ $\mathrm{mol}$ ${\mathrm{L}}^{-1}$ ${\mathrm{s}}^{-1}$
$4.$ $4.27$ $\times$ ${10}^3$ $\mathrm{mol}$ ${\mathrm{L}}^{-1}$ ${\mathrm{s}}^{-1}$

A reaction is first-order with respect to A and second-order with respect to B. The concentration of B is increased three times. The new rate of the reaction would: