The rate of a reaction is expressed in different ways as follows:

$+\frac{1}{2} \frac{d[C]}{d t}=-\frac{1}{5} \frac{d[D]}{d t}=+\frac{1}{3} \frac{d[A]}{d t}=-\frac{d[B]}{d t}$

Identify the reaction among the following:

1. 4𝐴 + 𝐵 → 2𝐶 + 3𝐷

2. 𝐵 + 5𝐷 → 3𝐴 + 2𝐶

3. 4A +2B →2C +3D

4.  B + \(\frac 12\)D → 4A →2C$$

For the reaction N₂ + 3H₂ $\to$ 2NH₃, the rate $\frac{\mathrm{d}\left[{\mathrm{NH}}_3\right]}{\mathrm{dt}}$ = 2x10^-4 Ms^-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

For a zero-order reaction:
2X + Y → Z

Which of the following represents the correct rate law?

For the reaction:
A + 2B → C + D

Which of the following statements is correct?

In the formation of sulphur trioxide by the contact process:

2SO₂(g) + O₂(g) $\to$2SO₃(g)

The rate of reaction is expressed as $\frac{\mathrm{d}\left[{\mathrm{O}}_2\right]}{\mathrm{dt}}$= 2.5×10^–4 mol L^–1 sec^–1. Find the rate of disappearance of SO₂ :

1. 5.0×10^–4 mol L^–1sec^–1

2. 2.5×10^–4 mol L^–1sec^–1

3. 3.75×10^–4 mol L^-1sec^–1

4. 50.0×10^–4 mol L^–1sec^–1

Compounds A and B react according to the following chemical equation.

A(g) + 2B(g) $\stackrel{}{\to }$ 2C(g)

The concentration of either A or B was changed keeping the concentrations of one of the reactants constant and rates were measured as a function of initial concentration. The following results were obtained. Choose the correct option for the rate equations for this reaction.