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A gaseous reaction $A_2\left(g\right) \to B\left(g\right) + \frac{1}{2}C\left(g\right)$ show increase pressure from 100 mm to
120 mm in 5 minutes. The rate of disappearance of (A${}_2$) will be 
1. 4 mm min ${}^{-1}$
2. 8 mm min${}^{-1}$ 
3. 16 mm min${}^{-1}$ 
4. 2 mm min${}^{-1}$

In a catalytic reaction, involving the formation of ammonia by Haber's process $N_2+3H_2\to 2N{H}_{3,}$ the rate of appearance of NH₃. was measured as $2.5\times {10}^{-4} mol L^{-1}{s}^{-1}$. The rate of disappearance of H₂ will be- 
1.  2.5 $\times$ 10${}^{-4}$ mol L${}^{-1}$ s${}^{-1}$
2. 1.25 $\times$ 10${}^{-4}$ mol L${}^{-1}$ s${}^{-1}$ 
3. 3.75 $\times$ 10${}^{-4}$ molL${}^{-1}$ s${}^{-1}$
4. 5.00 $\times$ 10${}^{-4}$ mol L${}^{-1}$ s${}^{-1}$

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 A${}_2$ + B${}_2$ $\to$2 A B occurs by the following mechanism 
$A_2 \to A+A$....... (slow) 
A +B${}_2$$\to$ AB + B....(fast) 
A+B$\to$AB......(fast)
Its order would be
1. 3/2 
2. 1
3. Zero 
4.2

Whcih of the following represents the expression for 3/4th life of a first order reaction?
1. $\frac{K}{2.303}\log \frac{4}{3}$
2.$\frac{2.303}{K}\log \frac{3}{4}$
3. $\frac{2.303}{K}\log 4$
4. $\frac{2.303}{K}\log 3$

For 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) 1 st 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 
l                     0.012                  0..035                0.1
ll                    0.024                   0.070                0.8
lll                   0.024                   0.035                0.1
lV                   0.012                   0.070                0.8
1. rate= k[B]${}^3$
2. rate= k[B]${}^4$
3. rate= k[A][B]${}^3$
4. rate= k[A]${}^2$ [B]${}^2$
 
 

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

The plot of log k vs $\frac{1}{T}$ 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.

Rate constant K= $1.2\times {10}^3$ mol L^-1 s^-1 and $E_a =2.0\times {10}^{2}KJ mo{l}^{-1}. When T\to \infty$, A is equal to 
(1) 2.0 $\times {10}^2\hspace{0.17em}mo{l}^{-1}{L}^{-1}{s}^{-1}$
(2) 1.2 $\times$ 10³ mol L^-1 s^-1
(3) 3.3 $\times$ 10³  mol L^-1 s^-1
(4) 2.4 $\times$ 10³ mol L^-1 s^-1

The reate constant for a reaction $2\times {10}^{-2}{s}^{-1}$at 300K and $8\times {10}^{-2}s-1$ at 340K. The
energy of activation of the  reaction is 
1. 14.695 KJ mol${}^{-1}$
2.  29.39 KJ mol${}^{-1}$ 
3. 44 KH mol${}^{-1}$
4. 22 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 the $∆$H 
2. Zero 
3. More than $∆$H 
4. Equal to $∆$H 

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 disappearance of ${\mathrm{NO}}_2$​, will be

When the concentration of reactant was made 4 times rate of reaction becomes 8 times. The order of reaction with respect to that reactant is 
1. 2
2. 3
3. 1
4. 1.5

What is the half of a radioactive substance if 87.5% of given amount disitegrates in 40
minutes?
1. 160 minutes 
2. 10 minutes
3. 20 minutes
4.13.33 minutes

If the temperature coefficient of a reaction is 3, to what factor the rate of raction
increases increase when temperature is increased from 30$°$ C to 60$°$ C?
1. 3
2. 6
3. 9 
4. 27

A gas phase reaction, R$\to$A+B+C+D is of first order. The initial pressure was P$°$ where
pressure after 10 minutes was P(P>P$°$). The corect expression for rate constant (K) is 
1. $K=\frac{2.303}{10}\log \frac{4°}{3P°-P}$
2. $K=\frac{2.303}{10}\log \frac{2P°}{3P°-P}$
3. $K=\frac{2.303}{10}\log \frac{3P°}{4P°-P}$
4. $K=\frac{2.303}{10}\log \frac{4P°}{4P°-P}$