It should be predicted that whether the given process that is Water vapour condenses as liquid water at 0 ° C and 1 atm pressure results in increase in entropy of the system or not. Concept introduction: The process is said to be spontaneous if the entropy change should increase and the value of change in free energy should be negative. Entropy increases in the order solid < liquid < gas . In the gaseous state, the particles are more random. In solids, the particles have fixed positions and entropy is less. In liquids, there are constraints due to forces between the particles. The increase in entropy results in a spontaneous process. Reactions that involve increased number of moles in a gaseous system results in increased entropy of the system.
Solution Summary: The author explains that the process is spontaneous if the entropy change should increase and the value of change in free energy should be negative.
Interpretation: It should be predicted that whether the given process that is Water vapour condenses as liquid water at 0 °C and 1 atm pressure results in increase in entropy of the system or not.
Concept introduction: The process is said to be spontaneous if the entropy change should increase and the value of change in free energy should be negative.
Entropy increases in the order solid < liquid < gas. In the gaseous state, the particles are more random. In solids, the particles have fixed positions and entropy is less. In liquids, there are constraints due to forces between the particles. The increase in entropy results in a spontaneous process.
Reactions that involve increased number of moles in a gaseous system results in increased entropy of the system.
(b)
Interpretation Introduction
Interpretation: It should be predicted that whether the given process that is exothermic reaction of Al(s) and Br2(l) in formation of Al2Br6(s) results in increase in entropy of the system or not.
Concept introduction: The process is said to be spontaneous if the entropy change should increase and the value of change in free energy should be negative.
Entropy increases in the order solid < liquid < gas. In the gaseous state, the particles are more random. In solids, the particles have fixed positions and entropy is less. In liquids, there are constraints due to forces between the particles. The increase in entropy results in a spontaneous process.
Reactions that involve increased number of moles in a gaseous system results in increased entropy of the system.
(c)
Interpretation Introduction
Interpretation: It should be predicted that whether the given process that is endothermic decomposition of solid CaCO3 results in increase in entropy of the system or not.
Concept introduction: The process is said to be spontaneous if the entropy change should increase and the value of change in free energy should be negative.
Entropy increases in the order solid < liquid < gas. In the gaseous state, the particles are more random. In solids, the particles have fixed positions and entropy is less. In liquids, there are constraints due to forces between the particles. The increase in entropy results in a spontaneous process.
Reactions that involve increased number of moles in a gaseous system results in increased entropy of the system.
(d)
Interpretation Introduction
Interpretation: It should be predicted that whether the given process that is decomposition of one mole of AgCl(s) to form 1.0 mole of Ag(s) and 0.5 mol of Cl2(g) results in increase in entropy of the system or not.
Concept introduction: The process is said to be spontaneous if the entropy change should increase and the value of change in free energy should be negative.
Entropy increases in the order solid < liquid < gas. In the gaseous state, the particles are more random. In solids, the particles have fixed positions and entropy is less. In liquids, there are constraints due to forces between the particles. The increase in entropy results in a spontaneous process.
Reactions that involve increased number of moles in a gaseous system results in increased entropy of the system.
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The Laws of Thermodynamics, Entropy, and Gibbs Free Energy; Author: Professor Dave Explains;https://www.youtube.com/watch?v=8N1BxHgsoOw;License: Standard YouTube License, CC-BY