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 ) 

1. 2.5 x 10^-4 mol L^-1 s^-1 and 5.5 x 10^-4 mol L^-1 s^-1

2. 2.5 x 10^-4 mol L^-1 s^-1 and 7.5 x 10^-4 mol L^-1 s^-1

3. 1.5 x 10^-4 mol L^-1 s^-1 and 4.5 x 10^-4 mol L^-1 s^-1

4. 0.5 x 10^-4 mol L^-1 s^-1 and 3.5 x 10^-4 mol L^-1 s^-1

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^-1min^-2  
4. bar^-1/2min^-1

The factor(s) that affect the rate of a chemical reaction is/are: 

1. Concentration/Pressure of reactants.

2. Temperature.

3. Presence of a catalyst. 

4. All of the above.

The correct statement about the rate constant of a reaction is:

$1.$ $6.67$ $\times {10}^{-2}$ $\mathrm{mol}$ ${\mathrm{L}}^{-1}$ ${\mathrm{s}}^{-1}$
$2.$ $2.67$ $\times$ ${10}^{-4}$ $\mathrm{mol}$ ${\mathrm{L}}^{-1}$ ${\mathrm{s}}^{-1}$ $$
$3.$ $4.67$ $\times$ ${10}^{-3}$ $\mathrm{mol}$ ${\mathrm{L}}^{-1}$ ${\mathrm{s}}^{-1}$
$4.$ $4.27$ $\times$ ${10}^3$ $\mathrm{mol}$ ${\mathrm{L}}^{-1}$ ${\mathrm{s}}^{-1}$

A reaction is first-order with respect to A and second-order with respect to B. The concentration of B is increased three times. The new rate of the reaction would:

In a reaction between A and B, the initial rate of reaction (r₀) was measured for different initial concentrations of A and B as given below:

The order of the reaction with respect to A and B would be:

For a reaction, 2A + B → C + D, the following observations were recorded:

The rate law applicable to the above mentioned reaction would be:

1. Rate = k[A]²[B]³

2. Rate = k[A][B]²

3. Rate = k[A]²[B]  

4. Rate = k[A][B]  

Given the following observations:

The reaction between A and B is first-order with respect to A and zero-order with respect to B. The values of X and Y are, respectively:

1.  X = 0.2 \(mol\) \(L^{- 1}\); Y = \(\) \(0 . 08\) \(mol\) \(L^{- 1} \left(min\right)^{- 1}\)

2.  X = 0.02 \(mol\) \(L^{- 1}\); Y = \(\) \(0 . 08\) \(mol\) \(L^{- 1} \left(min\right)^{- 1}\)

3.  X = 0.01 \(mol\) \(L^{- 1}\); Y = \(\) \(0 . 8\) \(mol\) \(L^{- 1} \left(min\right)^{- 1}\)

4. X = 0.2 \(mol\) \(L^{- 1}\); Y = \(\) \(0 . 8\) \(mol\) \(L^{- 1} \left(min\right)^{- 1}\)

The rate constant of a radioactive substance is $4$ ${\mathrm{years}}^{-1}$. The value of half-life will be : 

1. 0.05 years

2. 0.17 years

3. 0.26 ${\mathrm{years}}^{-1}$

4. 1.6 years