The reaction below is an example of:

CH₃COOC₂H₅   +   H₂O   \(\xrightarrow[]{H^{+}}\) CH₃COOH  +   C₂H₂OH
Ethyl acetate                           Acetic acid     Ethyl alcohol

${}_{}$

1. Pseudo-first-order reaction

2. First-order reaction

3. Second order reaction

4. Third-order reaction

What is the rate equation for reaction 2A+ B $\stackrel{}{\to }$ C if the order of the reaction is zero ?

1.$k {\left[A\right]}^{0 }{\left[B\right]}^0$

2. $k {\left[A\right]}^1{\left[B\right]}^0$

3. $k {\left[A\right]}^1{\left[B\right]}^1$

4. None of these

For a certain reaction large fraction of molecules have energy more than the threshold energy, yet why the rate of reaction is very slow.It is due to improper: 

1. Orientation of colliding molecules.

2. Energy of colliding molecules.

3. Volume of colliding molecules.

4. Entropy of colliding molecules.

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:

In a reaction with second-order kinetics where molecules X convert to Y, increasing the concentration
of X to three times its original value will affect the rate of Y formation by which factor?

1. 6 times

2. 9 times

3. 12 times

4. 3 times

The rate of a chemical reaction doubles when the temperature increases by 10 K (from 298 K). What is the activation energy of the reaction?

1. 65.6 Jmol^-1

2. 52.9 kJmol^-1

3. 45.9 kJmol^-1

4. 35.7 Jmol^-1

The activation energy for the reaction 2HI(g) → H₂(g)+ I₂(g) is 209.5 kJ mol⁻¹ at 581K. What is the fraction of molecules of reactants having energy equal to or greater than activation energy?

$1. 2.31 \times {10}^{-16}$
$2. 3.52 \times {10}^{-18}$
$3. 1.47 \times {10}^{-19}$
$4. 2.13 \times {10}^{-20}$

The rate constant for a first order reaction is 60 s^–1. How much time will it take to reduce the initial concentration of the reactant to its 1/16^th value?

$1. 2.3 \times {10}^{-2} \mathrm{s}$
$2. 4.6 \times {10}^{-2 }\mathrm{s}$
$3. 3.1 \times {10}^{-3} \mathrm{s}$
$4. 1.4 \times {10}^{-2} \mathrm{s}$

A first-order reaction takes 40 min for 30 % decomposition. The half life of the reaction will be: 

The rate constant for the decomposition of hydrocarbons is 2.418 × 10^–5 s^–1 at 546 K. If the energy of activation is 179.9 kJ/mol, the value of the pre-exponential factor will be:
1. $4.0$ $\times$ ${10}^{12}$ ${\mathrm{s}}^{-1}$
2. $7.8$ $\times$ ${10}^{-13}$ ${\mathrm{s}}^{-1}$
3. $3.8$ $\times$ ${10}^{-12}$ ${\mathrm{s}}^{-1}$
4. $4.7$ $\times$ ${10}^{12}$ ${\mathrm{s}}^{-1}$