Rate constant K = 1.2×10³ mol^–1 L s^–1 and E_a = 2.0×10² kJ mol^–1. When T $\to \infty$ , A is equal
to
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 reaction 2A + B + C $\to$ D + E is found to be a first-order reaction with respect to A, second-order reaction with respect to B, and zero-order reaction with respect to C. If the concentrations of A, B, and C are doubled, the rate of the reaction will be:

1. 72 times

2. 8 times

3. 24 times

4. 36 times

Zieglar-Natta catalyst is

1.  $\mathrm{K}\left[{\mathrm{PtCl}}_3\left({\mathrm{C}}_2{\mathrm{H}}_4\right)\right]$

2.  ${\left({\mathrm{Ph}}_3\mathrm{P}\right)}_3\mathrm{RhCl}$

3.  ${\mathrm{Al}}_2{\left({\mathrm{C}}_2{\mathrm{H}}_5\right)}_6+{\mathrm{TiCl}}_4$

4.  $\mathrm{Fe}{\left({\mathrm{C}}_5{\mathrm{H}}_5\right)}_2$

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.

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 first-order reaction has a rate constant of 2.303$\times {10}^{-3}$ ${\mathrm{s}}^{-1}$. The time required for 40 g of this reactant to reduce to 10 g will be
[Given that ${\log }_{10}2=0.3010$]

For a reaction, activation energy $E_a=0$ and the rate constant at 200 K is    1.6 $\times$ ${10}^6{s}^{-1}$. The rate constant at 400K will be [Given that gas constant, R=8.314 J $K^{-1}$ $mo{l}^{-1}$]

1.  3.2 × 10⁴ s^-1
2. 1.6 × 10⁶s^-1
3. 1.6 × 10³ s^-1
4. 3.2 × 10⁶ s^-1

The activation energies of two reactions are ${\mathrm{E}}_{{\mathrm{a}}_1}$ and ${\mathrm{E}}_{{\mathrm{a}}_2}$ with  ${\mathrm{E}}_{{\mathrm{a}}_1}$ > ${\mathrm{E}}_{{\mathrm{a}}_2}$.
f the temperature of the reacting system is increased from T₁ to T₂ .
The correct relation is: 

1. $\frac{{\mathrm{K}}_1\text{'}}{{\mathrm{K}}_1}=\frac{{\mathrm{K}}_2\text{'}}{{\mathrm{K}}_2}$         

2. $\frac{{\mathrm{K}}_1\text{'}}{{\mathrm{K}}_1}>\frac{{\mathrm{K}}_2\text{'}}{{\mathrm{K}}_2}$

3. $\frac{{\mathrm{K}}_1\text{'}}{{\mathrm{K}}_1}<\frac{{\mathrm{K}}_2\text{'}}{{\mathrm{K}}_2}$         

4. $\frac{{\mathrm{K}}_1\text{'}}{{\mathrm{K}}_1}<2\frac{{\mathrm{K}}_2\text{'}}{{\mathrm{K}}_2}$

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

1.  757.48 K

2.  378.74 K

3.  600.91 K

4.  None of the above