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

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.

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

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