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:

The conversion of molecules X to Y follows second order kinetics. If concentration of X is increased to three times how will it affect the rate of formation of Y?

1. 6 times

2. 9 times

3. 12 times

4. 3 times

The rate of the chemical reaction doubles for an increase of 10 K in absolute temperature from 298 K. The activation energy of the chemical reaction is ?

1. 55.6 Jmol^-1

2. 45.6 kJmol^-1

3. 52.9 kJmol^-1

4. 45.7 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:

$1.$ $4.0$ $\times$ ${10}^{12}$ ${\mathrm{s}}^{-1}$
$2.$ $7.8$ $\times$ ${10}^{-13}$ ${\mathrm{s}}^{-1}$
$3.$ $3.8$ $\times$ ${10}^{-12}$ ${\mathrm{s}}^{-1}$
$4.$ $4.7$ $\times$ ${10}^{12}$ ${\mathrm{s}}^{-1}$

For a reaction A → Product, with k = 2.0 × 10^–2 s^–1, if the initial concentration of A is 1.0 mol L^-1, the concentration of A after 100 seconds would be :