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Chapter 14: Problem 3

What are the advantages of measuring the initial rate of a reaction?

Short Answer

Expert verified
The advantages of measuring the initial rate of a reaction include: 1) accurate determination of the reaction rate, 2) gaining insight into the reaction mechanism, and 3) enabling manipulation of reaction conditions for optimal results.

Step by step solution

01

Understanding the Concept

The initial rate of a reaction refers to the change in concentration of a reactant or a product per unit time at the start of the reaction - essentially, the speed at which a reaction proceeds when it just begins. This rate can be measured before the reaction reaches equilibrium.
02

Advantage 1: Accurate Determination of Reaction Rate

One advantage of measuring the initial rate of a reaction is that it leads to an accurate determination of the reaction rate. Since measurements are taken before the reaction starts to slow down due to depletion of reactants, it eliminates the influence of back reactions or side reactions.
03

Advantage 2: Insight into Reaction Mechanism

Measuring the initial rate of reaction helps to understand the reaction mechanism. It allows one to infer how reactants are transformed into products step-by-step by understanding the order of reaction, which can provide insight into the sequence of steps that make up the overall reaction.
04

Advantage 3: Enabling Manipulation of Reaction Conditions

Understanding the initial rate can enable scientists to manipulate the reaction conditions such as concentration of reactants, temperature etc., for desired speed and results. It aids in designing efficient industrial processes by optimizing reaction conditions for maximum yield at minimal cost.

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Most popular questions from this chapter

Which of these species cannot be isolated in a reaction: activated complex, product, intermediate?

Suggest experimental means by which the rates of the following reactions could be followed: (a) \(\mathrm{CaCO}_{3}(s) \longrightarrow \mathrm{CaO}(s)+\mathrm{CO}_{2}(g)\) (b) \(\mathrm{Cl}_{2}(g)+2 \mathrm{Br}^{-}(a q) \longrightarrow \mathrm{Br}_{2}(a q)+2 \mathrm{Cl}^{-}(a q)\) (c) \(\mathrm{C}_{2} \mathrm{H}_{6}(g) \longrightarrow \mathrm{C}_{2} \mathrm{H}_{4}(g)+\mathrm{H}_{2}(g)\)

Sketch a potential-energy-versus-reaction-progress plot for the following reactions: $$ \begin{array}{l} \text { (a) } \mathrm{S}(s)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{SO}_{2}(g) \\ \Delta H^{\circ}=-296.06 \mathrm{~kJ} / \mathrm{mol} \\ \text { (b) } \mathrm{Cl}_{2}(g) \longrightarrow \mathrm{Cl}(g)+\mathrm{Cl}(g) \\\ \Delta H^{\circ}=242.7 \mathrm{~kJ} / \mathrm{mol} \end{array} $$

Define the half-life of a reaction. Write the equation relating the half-life of a first-order reaction to the rate constant.

What is the molecularity of a reaction?
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