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For the reaction, $2{\mathrm{NO}}_2\underset{{\mathrm{K}}_2}{\overset{{\mathrm{K}}_1}{\rightleftharpoons }}{\mathrm{N}}_2{\mathrm{O}}_4$, the rate law for the disappearence of ${\mathrm{NO}}_2$ will be
1. ${\mathrm{K}}_1{\left[{\mathrm{NO}}_2\right]}^2-{\mathrm{K}}_2\left[{\mathrm{N}}_2{\mathrm{O}}_4\right]$
2. $2{\mathrm{K}}_1{\left[{\mathrm{NO}}_2\right]}^2-2{\mathrm{K}}_2\left[{\mathrm{N}}_2{\mathrm{O}}_4\right]$
3. $2{\mathrm{K}}_1{\left[{\mathrm{NO}}_2\right]}^2-{\mathrm{K}}_2\left[{\mathrm{N}}_2{\mathrm{O}}_4\right]$
4. ${\mathrm{K}}_1{\left[{\mathrm{NO}}_2\right]}^2-2{\mathrm{K}}_2\left[{\mathrm{N}}_2{\mathrm{O}}_4\right]$

In a catalytic reaction involving the formation of ammonia by Haber’s process ${\mathrm{N}}_2+3{\mathrm{H}}_2\to 2{\mathrm{NH}}_3$, the rate of appearence of ${\mathrm{NH}}_3$ was measured as $2.5\times {10}^{-4}<mspace\; width="1em"></mspace>\mathrm{mol}<mspace\; width="1em"></mspace>{\mathrm{L}}^{-1}{\mathrm{s}}^{-1}$.The rate of disappearance of H₂ will be
1. 2.5×10^–4 mol L^–1s^–1
2. 1.25×10^–4 mol L^–1s^–1
3. 3.75×10^–4 mol L^–1s^–1
4. 5.00×10^–4 mol L^–1s^–1

For a chemical reaction, A $\to$ products, the rate of reaction doubles when the concentration of
A is increased by 4 times. The order of reaction is
1. 4
2. 0
3. 1/2
4. 1

The units of rate constant and rate of reaction are same for :
1. First order reaction
2. Second order reaction
3. Third order reaction
4. Zero order reaction

A reaction ${\mathrm{A}}_2+{\mathrm{B}}_2\to 2\mathrm{AB}$ occurs by the
following mechanism
${\mathrm{A}}_2\to \mathrm{A}+\mathrm{A}....\left(\mathrm{slow}\right)$
$\mathrm{A}+{\mathrm{B}}_2\to \mathrm{AB}+\mathrm{B}....\left(\mathrm{fast}\right)$
$\mathrm{A}+\mathrm{B}\to \mathrm{AB}....\left(\mathrm{fast}\right)$
Its order would be
1. 3/2
2. 1
3. Zero
4. 2

Which of the following represents the
expression for 3/4th life of a first order reaction?
1. $\frac{\mathrm{k}}{2.303}\log \frac{4}{3}$
2. $\frac{2.303}{\mathrm{k}}\log \frac{3}{4}$
3. $\frac{2.303}{\mathrm{k}}\log <mspace\; width="1em"></mspace>4$
4. $\frac{2.303}{\mathrm{k}}\log <mspace\; width="1em"></mspace>3$

For a reaction X(g) $\to$ Y(g) + Z(g), the half life
period is 10 min. In what period of time would
the conenctration of X be reduced to 10% of
original concentration
1. 20 min
2. 33 min
3. 15 min
4. 25 min

The hydrolysis of ester is alkaline medium is a
1. 1st order reaction with molecularity 1
2. 1st order reaction with molecularity 2
3. 2nd order reaction with molecularity 1
4. 2nd order reaction with molecularity 2

Select the law that corresponds to data shown
for the following reaction A + B  Products
Exp.     [A]           [B]           Intial rate
1        0.012       0.035         0.1
2        0.024       0.070         0.8
3        0.024       0.035         0.1
4        0.012       0.070         0.8
1. $\mathrm{rate}=\mathrm{k}{\left[\mathrm{B}\right]}^3$
2. $\mathrm{rate}=\mathrm{k}{\left[\mathrm{B}\right]}^4$
3. $\mathrm{rate}=\mathrm{k}\left[\mathrm{A}\right]{\left[\mathrm{B}\right]}^3$
4. $\mathrm{rate}=\mathrm{k}{\left[\mathrm{A}\right]}^2{\left[\mathrm{B}\right]}^2$

The activation energy for the forward reaction
X$\to$Y is 60kJ mol–1 and $∆$H is –20kJ mol^–1, the
activation energy for the reverse recation is
1. 40kJ mol^–1
2. 60kJ mol^–1
3. 80kJ mol^–1
4. 20kJ mol^–1

The plot of log k vs $\frac{1}{\mathrm{T}}$ helps to calculate : 
1. Energy of activation.
2. Rate constant of reaction.
3. Order of the reaction.
4. Energy of activation as well as the frequency factor.

Which of the following represents the value of the pre-exponential factor (A) for a reaction when the rate constant is K = 1.2×10³ mol^–1 L s^–1 and activation energy E_a = 2.0×10² kJ mol^–1, in the limit \(T→∞\)?
1. 2.0 × 10² kJ mol^–1
2. 1.2 × 10³ mol^–1L s^–1
3. 1.2 × 10³ mol L^–1 s^–1
4. 2.4 × 10³ kJ mol^–1L s^–1

The rate constant for a reaction 2×10^–2 s^–1 at 300 K and 8×10^–2 s^–1 at 340 K. The energy of activation of the reaction is:
1. 14.69 kJ mol^–1
2. 29.39 kJ mol^–1
3. 44.34 kJ mol^–1
4. 22.05 kJ mol^–1

The effect of a catalyst in a chemical reaction is
to change the
1. Acivation energy
2. Equilibrium concentration
3. Heat of reaction
4. Final products

For an endothermic reaction, where $∆$H represents the enthalpy of the reaction in kJ/mol, the minimum value for the energy of activation will be
1. Less than $∆$ H
2. Zero
3. More than $∆$ H
4. Equal to $∆$ H