The experimental data for the reaction \(2 A + B_2 \longrightarrow 2 AB\) is The rate equation for the above data is
Exp. [A] \([B_2]\) Rate \((M\,s^{-1})\) 1 0.50 0.50 \(1.6 \times 10^{-4}\) 2. 0.05 1.00 \(3.2 \times 10^{-4}\) 3. 1.00 1.00 \(3.2 \times 10^{-4}\)
The experimental data for the reaction \(2 A + B_2 \longrightarrow 2 AB\) is The rate equation for the above data is
| Exp. | [A] | \([B_2]\) | Rate \((M\,s^{-1})\) |
|---|---|---|---|
| 1 | 0.50 | 0.50 | \(1.6 \times 10^{-4}\) |
| 2. | 0.05 | 1.00 | \(3.2 \times 10^{-4}\) |
| 3. | 1.00 | 1.00 | \(3.2 \times 10^{-4}\) |
- rate = k $[B_2]$
- rate = k $[B_2]^2$
- rate = k $[A]^2[B]^2$
- rate = k $[A]^2[B]$
The Correct Option is A
Solution and Explanation
Consider the following rate law equation,
\(\hspace15mm \frac{dx}{dt}=k [A]^m [B_2]^n\)
\(\, \, \, \, \, \, \, 1.6 \times 10^{-4}=k [0.50]^m [0.50]^n \hspace20mm ...(i)\)
\(\, \, \, \, \, \, \, 3.2 \times 10^{-4}=k [0.50]^m [1.0]^n \hspace20mm ...(ii)\)
\(\, \, \, \, \, \, \, 3.2 \times 10^{-4}=k [1.00]^m [1.0]^n \hspace20mm ...(iii)\)
From Eqs. (ii) and (iii)
\(\, \, \, \, \, \, \, \, \frac{3.2 \times 10^{-4}}{3.2 \times 10^{-4}}=\frac{k [1.00]^m [1.0]^n}{k [0.50]^m [1.0]^n}\)
\(\, \, \, \, \, \, \, \, \, \, \, \, 1 =2^m \, \, \, \, or \, \, \, \, 2^0=2^m\)
\(\therefore \, \, \, \, \, \, \, \, \, \, \, \, \, \, \, \, \, m=0\)
From Eqs. (i) and (ii)
\(\, \, \, \, \, \, \, \, \frac{3.2 \times 10^{-4}}{1.6 \times 10^{-4}}=\frac{k [0.50]^m [1.0]^n}{k [0.50]^m [0.50]^n}\)
\(\, \, \, \, \, \, \, \, \, \, \, \, \, \, \, 2= 2^n\)
or \(\, \, \, \, \, \, \, \, \, \, \, \, \, 2^1=2^n\)
\(\therefore \, \, \, \, \, \, \, \, \, \, n=1\)
Hence, rate
\(\hspace15mm \big(\frac{dx}{dt}\big)=k [A]^0 [B_2]^1\)
\(\hspace25mm =k [B_2]\)
The pace at which reactants are changed into products is known as the reaction rate or rate of reaction. The rate at which chemical reactions take place varies greatly. While some chemical processes achieve their ultimate equilibrium very instantly, others take longer.
A broad meaning of the term "reaction rate" is the pace at which a reaction occurs. For instance, the oxidation of iron has a low response rate because the process is long, but burning wood has a high reaction rate because the process is quick.
Consider a chemical reaction.
aA + bB → cC + dD
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a, b, d, d denotes stoichiometric coefficients.
According to the IUPAC, the reaction rate r, which takes place in a closed system without the formation of reaction intermediates under isochoric conditions, is defined as:
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Concepts Used:
Chemical Kinetics
Chemical kinetics is the description of the rate of a chemical reaction. This is the rate at which the reactants are transformed into products. This may take place by abiotic or by biological systems, such as microbial metabolism.
Rate of a Chemical Reaction:
The speed of a reaction or the rate of a reaction can be defined as the change in concentration of a reactant or product in unit time. To be more specific, it can be expressed in terms of: (i) the rate of decrease in the concentration of any one of the reactants, or (ii) the rate of increase in concentration of any one of the products. Consider a hypothetical reaction, assuming that the volume of the system remains constant. R → P
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Factors Affecting The Reaction Rate:
- The concentration of Reactants - According to collision theory, which is discussed later, reactant molecules collide with each other to form products.
- Nature of the Reactants - The reaction rate also depends on the types of substances that are reacting.
- Physical State of Reactants - The physical state of a reactant whether it is solid, liquid, or gas can greatly affect the rate of change.
- Surface Area of Reactants - When two or more reactants are in the same phase of fluid, their particles collide more often than when either or both are in the solid phase or when they are in a heterogeneous mixture. In a heterogeneous medium, the collision between the particles occurs at an interface between phases. Compared to the homogeneous case, the number of collisions between reactants per unit time is significantly reduced, and so is the reaction rate.
- Temperature - If the temperature is increased, the number of collisions between reactant molecules per second. Increases, thereby increasing the rate of the reaction.
- Effect Of Solvent - The nature of the solvent also depends on the reaction rate of the solute particles.
- Catalyst - Catalysts alter the rate of the reaction by changing the reaction mechanism.