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Chapter 8: Problem 172

In the following question two statements Assertion (A) and Reason (R) are given Mark. a. If \(\mathrm{A}\) and \(\mathrm{R}\) both are correct and \(\mathrm{R}\) is the correct explanation of \(\mathrm{A}\); b. If \(A\) and \(R\) both are correct but \(R\) is not the correct explanation of \(\mathrm{A}\); c. \(\mathrm{A}\) is true but \(\mathrm{R}\) is false; d. \(\mathrm{A}\) is false but \(\mathrm{R}\) is true, e. \(\mathrm{A}\) and \(\mathrm{R}\) both are false. (A): \(2 \mathrm{FeCl}_{3}+\mathrm{SnCl}_{2} \rightarrow \mathrm{FeCl}_{2}+\mathrm{SnCl}_{4}\) is a \(3^{\text {nd }}\) order reaction ( \(\mathbf{R}\) ): The rate constant for third order reaction has unit \(\mathrm{L}^{2} \mathrm{~mol}^{-2} \mathrm{~s}^{-1}\).

Short Answer

Expert verified
b. Both A and R are correct, but R is not the explanation for A.

Step by step solution

01

Analyzing Assertion (A)

The reaction given is \(2 \mathrm{FeCl}_{3}+\mathrm{SnCl}_{2} \rightarrow \mathrm{FeCl}_{2}+\mathrm{SnCl}_{4}\). To determine the order, normally experimental data is used. However, if the order is given or hypothesized, we will need to accept that the order can be different than the stoichiometric coefficients in the balanced equation. The assertion claims it is a third order reaction.
02

Analyzing Reason (R)

The reason provided states that the unit of the rate constant for a third order reaction is \(\mathrm{L}^{2} \mathrm{~mol}^{-2} \mathrm{~s}^{-1}\). For a reaction of order \(n\), the rate constant \(k\) will indeed have units \(\mathrm{mol}^{1-n} \mathrm{~L}^{n-1} \mathrm{~s}^{-1}\). Therefore, if \(n = 3\), the units are correctly given as \(\mathrm{L}^{2} \mathrm{~mol}^{-2} \mathrm{~s}^{-1}\).
03

Evaluating the Truth of Each Statement

Both statements are true: the reaction can be claimed as a third-order (even without experimental confirmation, as per problem context). The reason correctly states the units for the rate constant.
04

Establishing the Relationship

To determine if Reason (R) is the correct explanation for Assertion (A), consider the content. While Reason (R) is a correct statement about third-order reaction rate constants, it doesn't explain why the given reaction is third order. The order of a reaction is determined experimentally.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Rate Constant Units
The rate constant is an essential component in the study of reaction kinetics. Each reaction order has a distinctive unit for its rate constant. This unit helps to balance the equation that represents the rate of a chemical reaction. - First-order reactions have a rate constant with units of \(s^{-1}\). - Second-order reactions are characterized by units of \(mol^{-1} \ L \ s^{-1}\). - Third-order reactions, as described in the exercise, have rate constant units of \(L^{2} \, mol^{-2} \, s^{-1}\). These units are crucial as they ensure the rate equation is dimensionally consistent. When analyzing the reaction \(2 \text{FeCl}_3 + \text{SnCl}_2 \rightarrow \text{FeCl}_2 + \text{SnCl}_4\), the understanding of units confirms the nature and order of the reaction.
Chemical Reactions
Chemical reactions involve the transformation of reactants into products through various processes. The exercise showcases a redox reaction where ferric chloride \(\text{FeCl}_3\) reacts with tin(II) chloride \(\text{SnCl}_2\) to form ferrous chloride \(\text{FeCl}_2\) and tin(IV) chloride \(\text{SnCl}_4\). Understanding such reactions involves recognizing: - Reactants and products - Stoichiometric coefficients - Conditions necessary for the reaction to occur Identifying the order of a reaction helps determine how reactant concentration affects the rate. Orders are often inferred from stoichiometry but are formally determined through experimentation. In this example, the assertion of third-order suggests a complex interplay between molecules.
Physical Chemistry
Physical chemistry bridges the theory of chemistry with the principles of physics, exploring how they impact chemical reactions. This field covers thermodynamics, quantum chemistry, and kinetics鈥攖he latter being our main focus here. In the kinetic study of reactions: - Reaction order is derived from concentration studies. - Rate laws are formulated, defining the speed of reactions in relation to the concentration of reactants. Physical chemistry enables scientists to predict and control reaction conditions, achieving efficient chemical production. The discussed reaction is an excellent showcase for how theoretical principles guide practical applications, providing insights into molecular interactions and energetics.
IIT JEE Chemistry
IIT JEE Chemistry is a crucial subject for students aspiring to enter top engineering institutes in India. The problem was designed to test understanding of reaction order and kinetics, prominent topics in this exam section. For success in IIT JEE Chemistry, students should concentrate on: - Comprehending reaction mechanisms and kinetics - Grasping fundamental principles of thermodynamics and equilibrium The key is to integrate theoretical knowledge with practical problem-solving skills. Understanding complex topics like reaction order empowers students to tackle diverse questions, boosting performance in competitive exams. In essence, the exercise revolves around fundamental concepts that are vital for excelling in IIT JEE Chemistry.

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Most popular questions from this chapter

The rate law for the reaction \(\mathrm{RCl}+\mathrm{NaOH}\) (aq) \(\rightarrow \mathrm{ROH}+\mathrm{NaCl}\) is given by Rate \(=\mathrm{k}[\mathrm{RCl}] .\) The rate of the reaction will be a. Doubled on doubling the concentration of sodium hydroxide b. Halved on reducing the concentration of alkyl halide to one half c. Decreased on increasing the temperature of reaction d. Unaffected by increasing the temperature of the reaction.

Hydrogen iodide decomposes at \(800 \mathrm{~K}\) via a second order process to produce hydrogen and iodine according to the following chemical equation. \(2 \mathrm{HI}(\mathrm{g}) \rightarrow \mathrm{H}_{2}(\mathrm{~g})+\mathrm{I}_{2}(\mathrm{~g})\) At \(800 \mathrm{~K}\) it takes 142 seconds for the initial concentration of \(\mathrm{HI}\) to decrease from \(6.75 \times 10^{-2} \mathrm{M}\) to \(3.50 \times 10^{-2} \mathrm{M}\). What is the rate constant for the reaction at this temperature? a. \(6.69 \times 10^{-3} \mathrm{M}^{-1} \mathrm{~s}^{-1}\) b. \(7.96 \times 10^{-2} \mathrm{M}^{-1} \mathrm{~s}^{-1}\) c. \(19.6 \times 10^{-3} \mathrm{M}^{-1} \mathrm{~s}^{-1}\) d. \(9.69 \times 10^{-2} \mathrm{M}^{-1} \mathrm{~s}^{-1}\)

A mechanism for a naturally occurring reaction that destroys ozone is Step I: \(\mathrm{O}_{3}(\mathrm{~g})+\mathrm{HO}(\mathrm{g}) \rightarrow \mathrm{HO}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g})\) Step II: \(\mathrm{HO}_{2}(\mathrm{~g})+\mathrm{O}(\mathrm{g}) \rightarrow \mathrm{HO}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{~g})\) Which species is a catalyst and what type of catalysis is occurring? a. \(\mathrm{HO}_{2}\), heterogeneous b. \(\mathrm{HO}_{2}\), homogeneous c. HO, homogeneous d. HO, heterogeneous

If the volume of the vessel in which the reaction \(2 \mathrm{NO}+\mathrm{O}_{2} \rightarrow 2 \mathrm{NO}_{2}\) is occurring is diminished to \(1 / 3 \mathrm{rd}\) of its initial volume. The rate of the reaction will be increased by a. 5 times b. 8 times c. 27 times d. 35 times

For this reaction \(\mathrm{X}^{-}+\mathrm{OH}^{-} \rightarrow \mathrm{X}^{-}+\mathrm{XO}^{-}\)in an aque- ons medium, the rate of the reaction is given as \(\frac{\left(\mathrm{d}\left(\mathrm{XO}^{-}\right)\right.}{\mathrm{dt}}=\mathrm{K} \frac{\left[\mathrm{X}^{-}\right]\left[\mathrm{XO}^{-}\right]}{\left[\mathrm{OH}^{-}\right]}\) The overall order for this reaction is a. Zero b. 1 c. \(-1\) d. \(1 / 2\)
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