A reactant (A) forms two products :

$\mathrm{A}\stackrel{{\mathrm{k}}_1}{\to }\mathrm{B},<mspace\; width="1em"></mspace>\mathrm{Activation}<mspace\; width="1em"></mspace>\mathrm{Energy}<mspace\; width="1em"></mspace>{\mathrm{Ea}}_1$
$\mathrm{A}\stackrel{{\mathrm{k}}_2}{\to }\mathrm{C},<mspace\; width="1em"></mspace>\mathrm{Activation}<mspace\; width="1em"></mspace>\mathrm{Energy}<mspace\; width="1em"></mspace>{\mathrm{Ea}}_2$

If Ea₂ = 2 Ea₁, then k₁ and k₂ are related as:

1.	${\mathrm{k}}_2={\mathrm{k}}_1{\mathrm{e}}^{{\mathrm{Ea}}_1/\mathrm{RT}}$	2.	${\mathrm{k}}_2={\mathrm{k}}_1{\mathrm{e}}^{{\mathrm{Ea}}_2/\mathrm{RT}}$
3.	${\mathrm{k}}_1=k_2{\mathrm{e}}^{{\mathrm{Ea}}_1/R\mathrm{T}}$	4.	${\mathrm{k}}_1=2{\mathrm{k}}_2{\mathrm{e}}^{{\mathrm{Ea}}_2/\mathrm{KT}}$

NO₂ required for a reaction is produced by the decomposition of N₂O₅ in CCl₄ as per the equation,
2N₂O₅(g) $\to$ 4NO₂(g) + O₂(g)
The initial concentration of N₂O₅ is 3.00 mol L^–1 and it is 2.75 mol L^–1 after 30 minutes. The rate of formation of NO₂ is:
1. 2.083 × 10^–3 mol L^–1 min^-1
2. 8.333 × 10^–3 mol L^–1 min^-1
3. 4.167 ×10^–3 mol L^–1 min^-1
4. 1.667 × 10^–2 mol L^–1 min^-1

During a nuclear explosion, one of the products is ⁹⁰Sr with a half-life of 28.1 years. If 1µg of ⁹⁰Sr was absorbed in the bones of a newly born baby instead of calcium, the amount of ⁹⁰Sr that will remain after 10 years in the now grown up child would be -

(Given ,antilog(0.108)=1.28)

1. 0.227 µg 

2. 0.781 µg 

3. 7.81 µg 

4. 2.27 µg 

The rate equation of a reaction is expressed as, Rate = \(k(P_{CH_{3}OCH_{3}})^{\frac{3}{2}}\)

(Unit of rate = bar min^–1)

The units of the rate constant will be:
1. bar^1/2 min    
2. bar² min^–1   
3. bar^–1 min^–2  
4. bar^–1/2 min^–1

The decomposition of NH₃ on a platinum surface is a zero-order reaction. The rates of production of N₂ and H₂ will be respectively:
(given ; k = 2.5 × 10^–4 mol^–1 L s^–1 ) 

The half-life of a certain enzyme catalysed reaction is 138 s, that follow the 1st order kinetics. The time required for the concentration of the substance to fall from 1.28 mg L^–1 to 0.04 mg L^–1, is:

1. 276 s 

2. 414 s

3. 552 s 

4. 690 s

What does Z_AB represent in the collision theory of chemical reactions?

The half-life for a zero-order reaction having 0.02 M initial concentration of reactant is 100 s. The rate constant (in mol L^–1 s^–1) for the reaction is:

1. $1.0\times {10}^{-4}$

2. $2.0\times {10}^{-4}$

3. $2.0\times {10}^{-3}$

4. $1.0\times {10}^{-2}$

The plot of ln k vs \({1 \over T}\) for the following reaction, \(2N_2O_5(g) \rightarrow 4NO_2 (g) + O_2(g) \) gives a straight line with the slope of the line equal to \(-1.0 \times 10^4 K \).
What is the activation energy for the reaction in J mol^–1 ?
(Given: R = 8.3 J K^–1 mol^–1)