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Ch.19 - Chemical Thermodynamics
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All textbooksBrown 15th EditionCh.19 - Chemical ThermodynamicsProblem 26a

Chapter 19, Problem 26a

(a) Does the entropy of the surroundings increase for spontaneous processes?

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Hello. In this problem we are told that for a spontaneous reaction, the entropy of the surroundings will not change Grass. Is this statement true or false, recall that the change in entropy of the universe is equal to the change in entropy of the system. Plus the change in entropy of the surroundings. The change in entropy of the universe will be greater than zero. When we have an irreversible reaction that is spontaneous and the change in entropy of the universe will be equal to zero when we have a reversible reaction that is at equilibrium. So all we know about a spontaneous reaction is that change in entropy of the universe needs to be greater than zero. Change in entropy of the system and the surroundings are not known for certain without performing a calculation or carrying out an experiment. So the answer to this question then is false, which corresponds to answer B. Thanks for watching. Hope. This helped.
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Textbook Question

The element gallium (Ga) freezes at 29.8 °C, and its molar enthalpy of fusion is ΔHfus = 5.59 kJ/mol. (a) When molten gallium solidifies to Ga(s) at its normal melting point, is ΔS positive or negative?

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Textbook Question

The element gallium (Ga) freezes at 29.8 °C, and its molar enthalpy of fusion is ΔHfus = 5.59 kJ/mol. (b) Calculate the value of ΔS when 60.0 g of Ga(l) solidifies at 29.8 °C.

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Textbook Question

Indicate whether each statement is true or false. (c) In a certain spontaneous process the system undergoes an entropy change of 4.2 J/K; therefore, the entropy change of the surroundings must be -4.2 J/K.

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Textbook Question

(b) In a particular spontaneous process the entropy of the system decreases. What can you conclude about the sign and magnitude of ΔSsurr?

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Textbook Question

(c) During a certain reversible process, the surroundings undergo an entropy change, ΔSsurr = -78 J/K. What is the entropy change of the system for this process?

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Textbook Question

(a) What sign for Δ𝑆 do you expect when the pressure on 0.600 mol of an ideal gas at 350 K is increased isothermally from an initial pressure of 0.750 atm?

(b) If the final pressure on the gas is 1.20 atm, calculate the entropy change for the process.

(c) Which of the following statements about this process are true? (i) The entropy change you calculated will be the same for at any other constant temperature. (ii) The value of Δ𝑆 you calculated is valid only if the compression is done irreversibly. (iii) If the number of moles of gas being compressed were decreased by a factor of three, the entropy change would increase by a factor of three.