# Rate of Reaction Worksheet

The rate of reaction is used to describe the speed of reaction. It shows how fast or slow a reaction is taking place.

Chemical kinetics is used in-order to study the rate of reaction, which is a part of physical chemistry. The rate of reaction also depends upon the type of molecule that are combining.

Here, you can find some questions related to “Rate of reaction” and their answers:

Questions:

1. The rate of reaction is best defined as:

(a)    Change in the concentration of any one of th reactants or products per unit time

(b)   Decrease in the concentration of a reactant

(c)    Increase in the concentration of a product

(d)   All the three are correct

2. As the reaction progresses, the rate of reaction will:

(a)    Decreases

(b)   Increases

(c)    First increases, then decreases

(d)   Remain constant

3. Among the following reactions, the fastest rate is for:

(a)    Precipitation of silver chloride by mixing silver nitrate and sodium chloride solutions

(b)   Burning of charcoal

(c)    Rusting of iron in moist air

(d)   Conversion of nonoclinic sulphur to rhombic sulphur

4. Negative sign used in expressing the rate of reaction indicates:

(a)    The reaction is irreversible

(b)   There are attractive forces between the reactants

(c)    The rate is decreasing with time

(d)   The concentration of the reactant is decreasing with time

5. For the reaction $X + Y \to M + N$ the variation of the concentration of the product with time is given by the curve:

Rate of Reaction

(a)    A

(b)   B

(c)    C

(d)   D

6. Consider the chemical reaction $N_2 (g) + 3H_2 (g) \to NH_3 (g)$. The rate of this reaction can be expressed in terms of time derivative of concentration of$N_2 (g), H_2 (g) or NH_3 (g)$ .

Identify the correct relationship amongst the rate expressions:

$(a) \hspace{3mm} \text{Rate} = -d[N_2] /dt = -1/3 d [H_2]/dt \\[3mm] = 1/2 d[NH_3] /dt$

$(b) \hspace{3mm} \text{Rate} = -d[N_2]/dt = -3d[H_2]/dt \\[3mm] 2d[NH_3]/dt$

$(c) \hspace{3mm}\text{Rate} = - d[N_2] /dt = 1/3 d[H_2]/dt \\[3mm] = 1/2 d[NH_3]dt$

$(d) \hspace{3mm}\text{Rate} = -d[N_2]/dt = -d[H_2]/dt \\[3mm] = d[NH_3]/dt$

7. The rate of the reaction intermediates can be determined by the study of:

(a)    Catalyst effect

(b)   Concentration of the reactants

(c)    Temperature effects

(d)   Solvent effects

8. In the reversible reaction $2NO_2 \overset{K_1}{\underset{K_2} \rightleftharpoons} N_2O_4$ the rate of disappearance of $NO_2$ is equal to:

(a)    $\dfrac{2k_1}{k_2}[NO_2]^2$

(b)   $2k_1[NO_2]^2- 2k_2[N_2O_4]$

(c)    $2k_1[NO_2]^2- k_2[N_2O_4]$

(d)   $(2k_1- k_2)[NO_2]$

9. For a reaction: $2A + B \to \text{Products}$, the active mass of B is kept constant and that of A is doubled. The rate of reaction will then

(a)    Increases two times

(b)   Increases four times

(c)    Decreases two times

(d)   Decreases four times

10. For the reaction, $N_2 + 3H_2 \leftrightharpoons 2NH_3$  the rate of change of concentration for hydrogen is $-0.3 \times 10^{-4} m s^{-1}$.The rate of change of concentration of ammonia is:

(a)    $0.1 \times 10^{-4}$

(b)   $0.2 \times 10^{-4}$

(c)    $-0.2 \times 10^{-4}$

(d)   $0.3 \times 10^{-4}$

1.(a)      2. (a)     3. (a)     4. (d)     5. (b)

6. (a)     7. (b)     8. (b)     9. (b)     10. (b)

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