Textbook Question
Consider a process in which an ideal gas changes from state 1 to state 2 in such a way that its temperature changes from 300 K to 200 K. (b) Is this process isothermal?
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Ch.19 - Chemical Thermodynamics
Chapter 19, Problem 19
Consider a system consisting of an ice cube. (a) Under what conditions can the ice cube melt reversibly?
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Reversible Processes
A reversible process is a thermodynamic process that can be reversed without leaving any trace on the surroundings. In the context of melting ice, this means that the ice can transition to water and back to ice without any net change in the system or its environment. Reversible processes occur under specific conditions, typically involving equilibrium and infinitesimally slow changes.
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03:40
Reversible Changes in Matter
Phase Equilibrium
Phase equilibrium refers to the state in which multiple phases of a substance (like solid ice and liquid water) coexist at a specific temperature and pressure. For an ice cube to melt reversibly, it must be at the melting point (0°C at 1 atm) where the solid and liquid phases are in equilibrium. Any deviation from this equilibrium can lead to irreversible changes.
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03:22Phase Changes in Diagrams
Thermodynamic Conditions
The thermodynamic conditions, including temperature and pressure, play a crucial role in determining whether a phase change, such as melting, can occur reversibly. For an ice cube to melt reversibly, it must be subjected to conditions where the temperature is maintained at the melting point and the pressure is constant, allowing for the absorption of heat without changing the overall state of the system.
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01:18First Law of Thermodynamics
Related Practice
Textbook Question
Consider a process in which an ideal gas changes from state 1 to state 2 in such a way that its temperature changes from 300 K to 200 K. (c) Does the change in the internal energy, ΔE, depend on the particular pathway taken to carry out this change of state?
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Textbook Question
A system goes from state 1 to state 2 and back to state 1. (c) Suppose the changes in state are reversible processes. Is the work done by the system upon going from state 1 to state 2 the same or different as compared to that upon going from state 2 back to state 1?
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Textbook Question
Indicate whether each statement is true or false. (a) ΔS is a state function. (b) If a system undergoes a reversible change, the entropy of the universe increases. (c) If a system undergoes a reversible process, the change in entropy of the system is exactly matched by an equal and opposite change in the entropy of the surroundings. (d) If a system undergoes a reversible process, the entropy change of the system must be zero.
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Textbook Question
The normal boiling point of Br2(l) is 58.8 °C, and its molar enthalpy of vaporization is ΔHvap = 29.6 kJ/mol. (a) When Br2(l) boils at its normal boiling point, does its entropy increase or decrease?
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Textbook Question
The normal boiling point of Br2(𝑙) is 58.8 °C, and its molar enthalpy of vaporization is Δ𝐻vap=29.6 kJ/mol. (b) Calculate the value of Δ𝑆 when 1.00 mol of Br2(𝑙) is vaporized at 58.8 °C.
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