The rate of a chemical reaction primarily depends on which of the following factors?

1. Volume

2. Force

3. Pressure

4. Concentration of reactants

Following mechanism has been proposed for a reaction,

2A+B $\to$D+E

A+B$\to$ C+D    ...(Slow)

A+ C$\to$ E         ...(Fast)

The rate law expression for the reaction is:

1. r = K[A]²[B]

2. r=K[A][B]

3. r= K[A]²

4. r= K[A][C]

For the reaction N₂ + 3H₂ $\to$ 2NH₃, the rate $\frac{\mathrm{d}\left[{\mathrm{NH}}_3\right]}{\mathrm{dt}}$= 2 x 10^-4 M s^-1 .Therefore, the rate $\frac{-\mathrm{d}\left[{\mathrm{N}}_2\right]}{\mathrm{dt}}$ is given as:

1. 10^-4 Ms^-1

2. 10⁴ Ms^-1

3. 10^-2 sM^-1

4. 10^-4 sM^-1

When ethyl acetate was hydrolysed in pressure of 0.1 M HCl, the rate constant was found to be 5.40 x 10^-5 sec^-1 . But when 0.05 M H₂SO₄ was used for hydrolysis, the rate constant was found to be 6.25 X10^-5sec^-1. Thus, it may be concluded that:

1. H₂SO₄ is stronger than HCI

2. H₂SO₄ is weaker than HCl

3. H₂SO₄ and HCl both have the same strength

4. The data are not sufficient to compare the strength of H₂SO₄ and HCI

Find the correct rate law for the decomposition of ozone:

2O₃ → 3O₂

Mechanism:

O₃ ⇌ O₂ + O (Fast equilibrium)
O + O₃ → 2O₂ (Slow)

1. r = k[O₃]²
2. r = k[O₃]²[O₂]⁻¹
3. r = k[O₃][O₂]
4. Rate law cannot be predicted