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Chapter 19: Problem 31

(a) What do you expect for the sign of \(\Delta S\) in a chemical reaction in which two moles of gaseous reactants are converted to three moles of gaseous products? (b) For which of the processes in Exercise \(19.9\) does the entropy of the system increase?

Short Answer

Expert verified
For part (a), since the number of gaseous moles increases from 2 moles (reactants) to 3 moles (products), the overall randomness and dispersion of energy within the system have increased, resulting in a positive entropy change (鈭哠 > 0). For part (b), as Exercise 19.9 was not provided, the key criteria to check for an entropy increase are an increase in the number of particles, increased energy dispersion, and increased randomness of the system.

Step by step solution

01

(Part A: Entropy change sign determination)

For the given chemical reaction where two moles of gaseous reactants are converted to three moles of gaseous products, let's analyze the entropy change. Entropy (鈭哠) typically increases with an increase in the number of particles in the system. In this particular case, the number of gaseous moles increases from 2 moles (reactants) to 3 moles (products). Since the number of particles has increased, the overall randomness and dispersion of energy within the system have increased. Consequently, the entropy change (鈭哠) should be positive. So, we can expect a positive 鈭哠 for this reaction.
02

(Part B: Entropy increase in Exercise 19.9)

Exercise 19.9 is not provided. However, given a list of processes, we can determine whether the entropy would increase or not based on similar principles as discussed in Part A. Keep in mind that entropy increases when: 1. The number of particles in the system increases. 2. Energy dispersion is increased. 3. The randomness of the system increases (e.g., solid to liquid, liquid to gas). By analyzing the given processes in Exercise 19.9 based on these criteria, we can identify which processes will result in an increase in the entropy of the system.

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Most popular questions from this chapter

A particular reaction is spontaneous at \(450 \mathrm{~K}\). The enthalpy change for the reaction is \(+34.5 \mathrm{~kJ} .\) What can you conclude about the sign and magnitude of \(\Delta S\) for the reaction?

Explain qualitatively how \(\Delta G\) changes for each of the following reactions as the partial pressure of \(\mathrm{O}_{2}\) is increased: (a) \(2 \mathrm{CO}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{CO}_{2}(g)\) (b) \(2 \mathrm{H}_{2} \mathrm{O}_{2}(l) \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{O}_{2}(g)\) (c) \(2 \mathrm{KClO}_{3}(s) \longrightarrow 2 \mathrm{KCl}(s)+3 \mathrm{O}_{2}(g)\)

The normal freezing point of 1 -propanol \(\left(\mathrm{C}_{3} \mathrm{H}_{8} \mathrm{O}\right)\) is \(-127{ }^{\circ} \mathrm{C}\). (a) Is the freezing of 1-propanol an endothermic or exothermic process? (b) In what temperature range is the freezing of 1-propanol a spontaneous process? (c) In what temperature range is it a nonspontaneous process? (d) Is there any temperature at which liquid and solid 1-propanol are in equilibrium? Explain.

Acetylene gas, \(\mathrm{C}_{2} \mathrm{H}_{2}(g)\), is used in welding. (a) Write a balanced equation for the combustion of acetylene gas to \(\mathrm{CO}_{2}(g)\) and \(\mathrm{H}_{2} \mathrm{O}(l) .\) (b) How much heat is produced in burning \(1 \mathrm{~mol}\) of \(\mathrm{C}_{2} \mathrm{H}_{2}\) under standard conditions if both reactants and products are brought to \(298 \mathrm{~K} ?\) (c) What is the maximum amount of useful work that can be accomplished under standard conditions by this reaction?

Consider a reaction \(\mathrm{A}_{2}(g)+\mathrm{B}_{2}(g) \rightleftharpoons 2 \mathrm{AB}(g)\), with atoms of A shown in red and atoms of B shown in blue. (a) If \(K_{c}=1\), which system is at equilibrium? (b) What is the sign of \(\Delta G\) for any process in which the contents of a reaction vessel move to equilibrium? (c) Rank the boxes in order of increasing magnitude of \(\Delta G\) for the reaction. [Sections \(19.5\) and \(19.7]\)
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