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A hydrogenation reaction is carried out at 500 K. If the same reaction is carried out in the presence of a catalyst at the same rate with same frequency factor, the temperature required is 400 K. If the catalyst lowers the activation energy barrier by 16 kJ/mol then the activation energy of reaction is:
(1) 100 kJ/mol
(2) 80 kJ/mol
(3) 60 kJ/mol
(4) None of these

Consider the reaction.

The rate constant for two parallel reactions were found to be ${10}^{-2} {\mathrm{dm}}^3 {\mathrm{mol}}^{-1} {\mathrm{s}}^{-1}$ and $4\times {10}^{-2} {\mathrm{dm}}^3 {\mathrm{mol}}^{-1} {\mathrm{s}}^{-1}$. If the corresponding energy of activation of the parallel reaction are 100 and 120 kJ/mol respectively, The net energy of activation $\left({\mathrm{E}}_{\mathrm{a}}\right)$ of A is: 
(1) 150 kJ/mol
(2) 320 kJ/mol
(3) 116 kJ/mol
(4) 220 kJ/mol

A reaction takes place in various steps. The rate constant for first, second, third and fifth steps are ${\mathrm{k}}_1, {\mathrm{k}}_2, {\mathrm{k}}_3 \mathrm{and} {\mathrm{k}}_5$ respectively. The overall rate constant is given by , $\mathrm{k}=\frac{{\mathrm{k}}_2}{{\mathrm{k}}_3}{\left(\frac{{\mathrm{k}}_1}{{\mathrm{k}}_5}\right)}^{1/2}$
If activation energy are 40, 60, 50 and 10 kJ/mol respectively, the overall energy of activation (kJ/mol) is:
(1) 10
(2) 20
(3) 25
(4) None of the above.

For first order parallel reactions ${\mathrm{k}}_1 \mathrm{and} {\mathrm{k}}_2$ are 4  min^-1 and 2 $mi{n}^{-1}$ respectively at 300 K. If the activation energies for the formation of B and C are respectively 30,000 and 38,314 J/mol respectively, the temperature at which B and C will be obtained in equimolar ratio is:

(1) 757.48 K
(2) 378.74 K
(3) 600 K
(4) None of the above

For reaction A$\to$B, the rate constant ${\mathrm{k}}_1={\mathrm{A}}_1{\mathrm{e}}^{-{\mathrm{Ea}}_1/\left(\mathrm{RT}\right)}$ and for the reaction X$\to$Y, the rate constant ${\mathrm{k}}_2={\mathrm{A}}_2{\mathrm{e}}^{-{\mathrm{Ea}}_2/\left(\mathrm{RT}\right)}$. If ${\mathrm{A}}_1={10}^8, {\mathrm{A}}_2={10}^{10} \mathrm{and} {\mathrm{E}}_{{\mathrm{a}}_1}=600 \mathrm{cal}/\mathrm{mol},$ ${\mathrm{E}}_{{\mathrm{a}}_1}=1800 \mathrm{cal}/\mathrm{mol}$, then the temperature at which ${\mathrm{k}}_1={\mathrm{k}}_2$ is (Given: R=2 cal/K-mol)
(1) 1200 K
(2) 1200$\times$4.606 K
(3) $\frac{1200}{4.606} K$
(4) $\frac{600}{4.606} K$

Consider the plots, given below, for the types of reaction
nA$\to$B+C

These plots respectively correspond to the reaction orders:
1. 0, 1, 2
2. 1, 2, 0
3. 1, 0, 2
4. None of these

A graph between log $t_{1/2}$ and log a (abscissa), a being the initial concentration of A in the reaction for reaction A $\to$Product, the rate law is:

(1) $\frac{-\mathrm{d}\left[\mathrm{A}\right]}{\mathrm{dt}}=K$
(2) $\frac{-\mathrm{d}\left[\mathrm{A}\right]}{\mathrm{dt}}=K\mathit{\left[}A\mathit{\right]}$
(3) $\frac{-\mathrm{d}\left[\mathrm{A}\right]}{\mathrm{dt}}=K{\mathit{\left[}A\mathit{\right]}}^{\mathit{2}}$
(4) $\frac{-\mathrm{d}\left[\mathrm{A}\right]}{\mathrm{dt}}=K{\mathit{\left[}A\mathit{\right]}}^{\mathit{3}}$

For a zero order reaction, the plot of conc. (a-x) vs time is linear with
(1) +ve slope and zero intercept
(2) -ve slope and zero intercept
(3) +ve slope and non-zero intercept
(4) -ve slope and non-zero intercept

The kinetic data for the given reaction A(g) + 2B(g) $\stackrel{\mathrm{k}}{\to }$C(g) is provided in the following table for three experiments at 300 K

In another experiment starting with initial concentration of 0.5 and 1 M respectively for A and B at 300 K, find the rate of reaction after 50 minutes from the starting of experiment (in M/sec).
(1) $6.93\times {10}^{-4}$
(2) $0.25\times {10}^{-7}$
(3) $4.33\times {10}^{-5}$
(4) $3.46\times {10}^{-4}$

The following mechanism has been proposed for the exothermic catalyzed complex reaction
$\mathrm{A}+\mathrm{B}\underset{\mathrm{fast}}{\overset{\mathrm{slow}}{\rightleftharpoons }}\mathrm{IAB}\stackrel{{\mathrm{k}}_1}{\to }\mathrm{AB}+\mathrm{I}\stackrel{{\mathrm{k}}_2}{\to }\mathrm{P}+\mathrm{A}$
If ${\mathrm{k}}_1$ is much smaller than ${\mathrm{k}}_2$, the most suitable qualitative plot of potential energy (P.E.) versus reaction co-ordinate (R.C.) for the above reaction
(1)        
(2)
(3)      
(4)

The reaction A(g) + 2B(g)$\to$C(g) is an elementary reaction. In an experiment involving this reaction, the initial partial pressures of A and B are ${\mathrm{P}}_{\mathrm{A}}=0.40 \mathrm{atm} \mathrm{and} {\mathrm{P}}_{\mathrm{B}}=1.0 \mathrm{atm}$ respectively. When ${\mathrm{P}}_{\mathrm{C}}=0.3$ atm, the rate of the reaction relative to the initial rate is:
(1) $\frac{1}{12}$
(2) $\frac{1}{50}$
(3) $\frac{1}{25}$
(4) None of these

The forward rate constant for the elementary reversible gaseous reaction
${\mathrm{C}}_2{\mathrm{H}}_6\rightleftharpoons 2{\mathrm{CH}}_3 \mathrm{is} 1.57\times {10}^{-3} {\mathrm{s}}^{-1} \mathrm{at} 100 \mathrm{K}$
What is the rate constant for the backward reaction at this temperature if ${10}^{-4}$ moles of ${\mathrm{CH}}_3$ and 10 moles of ${\mathrm{C}}_2{\mathrm{H}}_6$ are present in a 10 litre vessel at equilibrium.
(1) $1.57\times {10}^9 \mathrm{L} {\mathrm{mol}}^{-1} {\mathrm{s}}^{-1}$
(2) $1.57\times {10}^{10} \mathrm{L} {\mathrm{mol}}^{-1} {\mathrm{s}}^{-1}$
(3) $1.57\times {10}^{11} \mathrm{L} {\mathrm{mol}}^{-1} {\mathrm{s}}^{-1}$
(4) $1.57\times {10}^7 \mathrm{L} {\mathrm{mol}}^{-1} {\mathrm{s}}^{-1}$

If decomposition reaction A(g)$\to$B(g) follows first order kinetics then the graph of rate of formation (R) of B against time t will be:
(1)     (2)
(3)     (4)

Decomposition of ${\mathrm{NH}}_4{\mathrm{NO}}_2\left(\mathrm{aq}\right)$ into ${\mathrm{N}}_2\left(\mathrm{g}\right) \mathrm{and} 2{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$ is first order reaction. Which of the following graph is correct?
(1)         (2)
(3)        (4)

A gaseous compound A reacts by three independent first order process (as shown in figure) with rate constant $2\times {10}^{-3}, 3\times {10}^{-3} \mathrm{and} 1.93\times {10}^{-3} {\sec }^{-1}$ for product B, C and D respectively. If initially pure A was taken in a closed container with P=8 atm, then the partial pressure of B (in atm) after 100 sec from starting the experiment,

(1) 0.288
(2) 0.577
(3) 1.154
(4) none of these