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For the elementary reaction M $\to$ N, the rate of disappearance of M increases by a factor of 8 upon doubling the concentration of M. The order of the reaction with respect to M will be:
1. 4
2. 3
3. 2
4. 1

The rate constant of a first-order reaction is\(4 \times 10^{-3} \mathrm{sec}^{-1}.\) At a reactant concentration of \(0.02~\mathrm{M},\) the rate of reaction would be:

For a first-order reaction A $\to$ Products, the rate of reaction at [A] = 0.2 M is 1.0 x 10^-2 mol litre^-1 min^-1. The half-life period for the reaction will be:

In the following reaction: xA →  yB
$\log \left(-\frac{d\left[A\right]}{d\mathrm{t<mspace\; width="1em"></mspace>}}\right)=$ $\log$ $\left(\frac{d\left[B\right]}{dt}\right)$ $+$ $0.3$ 
where the -ve sign indicates the rate of disappearance of the reactant. Then, x : y equals:

Half-life is independent of the concentration of a reactant. After 10 minutes, the volume of N₂ gas is 10 L and after complete reaction, it is 50 L. Hence, the rate constant is:
1. $\frac{2.303}{10}$log 5 min^-1
2. $\frac{2.303}{10}$ log 1.25 min^-1
3. $\frac{2.303}{10}$ log 2 min^-1
4. $\frac{2.303}{10}$ log 4 min^-1

A gaseous reaction A₂(g) → B(g) + $\frac{1}{2}C$(g) shows increase in pressure from 100 mm to 120 mm in 5 minutes. The rate of disappearance of A₂ will be : 

During the formation of ammonia by Haber's process N₂ + 3H₂ → 2NH₃, the rate of appearance of NH₃ was measured as 2.5 x 10^-4 mol L^-1 s^-1. The rate of disappearance of H₂ will be: 
1. 2.5 x 10^-4 mol L^-1 s^-1
2. 1.25 x 10^-4 mol L^-1 s^-1
3. 3.75 x 10^-4 mol L^-1 s^-1
4. 15.00 x 10^-4 mol L^-1 s^-1

During the kinetic study of the reaction, 2A + B → C + D, the following results were obtained:

Based on the above data, the correct rate law is:
1.  Rate=k[A]²[B]
2.  Rate=k[A][B]
3.  Rate=k[A]²[B]²
4.  Rate=k[A][B]²

A first-order reaction is 15 % completed in 20 minutes. The amount of time required to complete 60 % of the reaction is:

If ‘a’ is the initial concentration of a substance which reacts according to zero-order kinetics and k is the rate constant, the time for the reaction to go to completion will be:

For a given reaction the concentration of the reactant plotted against time gave a straight line with negative slope.
The order of the reaction will be:
1. 3                                                      
2. 2
3. 1                                                      
4. 0

If in the fermentation of sugar in an enzymatic solution that is 0.12 M, the concentration of the sugar is reduced to 0.06 M in 10 h and to 0.03 M in 20 h, the order of the reaction will be:
1. 1                                                   
2. 2
3. 3                                                   
4. 0

Which of the following statements about the order of reaction is incorrect?

If 60 % of a first-order reaction is completed in 60 minutes, 50 % of the same reaction takes approximately:
(log4 = 0.60, log5 = 0.69)

Select the correct option based on statements below:

${}_{}$
1. Pseudo-first-order reaction
2. First-order reaction
3. Second order reaction
4. Third-order reaction

For a general reaction A $\to$ B, the plot of the concentration of A vs. time is given in the figure.
 
The slope of the curve will be:

Consider the first-order gas-phase decomposition reaction given below.
A(g) → B(g) + C(g)
The initial pressure of the system before the decomposition of A was ${\mathrm{P}}_{\mathrm{i}}$. After the lapse of time t, the total pressure of the system increased by X units and became ${\mathrm{P}}_{\mathrm{t}}$. The rate constant k for the reaction is:

A first-order reaction is 50 % completed in 1.26 × 10¹⁴ s. The time required for 100 % completion of the reaction will be:
1. 1.26 × 10¹⁵ s
2. 2.52 × 10¹⁴ s
3. 2.52 × 10²⁸ s
4. Infinite

Match the graph given in Column I with the order of reaction given in Column II.
More than one item in Column I may be linked to the same item in Column II:

Column I		Column II
(i)		(a)	1st order
(ii)		(b)	Zero order
(iii)
(iv)