A non spontaneous process should be explained with an example. Concept introduction: As per second law of thermodynamics : • A process is called spontaneous when the entropy of the process increases so that ∆S is positive. The spontaneous processes takes place by own or by some initiation but they do not need any external force. For example fall of water from top level to bottom is spontaneous process. • A process is called non-spontaneous when the entropy of the process decreases so that ∆S is negative. Such processes need external force like heat or pressure to take place. They can neither occur by self or by initiation. For example; endothermic reactions are always non-spontaneous. Given:
A non spontaneous process should be explained with an example. Concept introduction: As per second law of thermodynamics : • A process is called spontaneous when the entropy of the process increases so that ∆S is positive. The spontaneous processes takes place by own or by some initiation but they do not need any external force. For example fall of water from top level to bottom is spontaneous process. • A process is called non-spontaneous when the entropy of the process decreases so that ∆S is negative. Such processes need external force like heat or pressure to take place. They can neither occur by self or by initiation. For example; endothermic reactions are always non-spontaneous. Given:
Solution Summary: The author explains that a non-spontaneous process can neither occur by self or by initiation.
Science that deals with the amount of energy transferred from one equilibrium state to another equilibrium state.
Chapter 19, Problem 3E
Interpretation Introduction
Interpretation:
A non spontaneous process should be explained with an example.
Concept introduction:
As per second law of thermodynamics:
• A process is called spontaneous when the entropy of the process increases so that ∆S is positive. The spontaneous processes takes place by own or by some initiation but they do not need any external force. For example fall of water from top level to bottom is spontaneous process.
• A process is called non-spontaneous when the entropy of the process decreases so that ∆S is negative. Such processes need external force like heat or pressure to take place. They can neither occur by self or by initiation.
For example; endothermic reactions are always non-spontaneous.
b) Certain cyclic compounds are known to be conformationally similar to carbohydrates, although they are not
themselves carbohydrates. One example is Compound C shown below, which could be imagined as adopting
four possible conformations. In reality, however, only one of these is particularly stable. Circle the conformation
you expect to be the most stable, and provide an explanation to justify your choice. For your explanation to be
both convincing and correct, it must contain not only words, but also "cartoon" orbital drawings contrasting the
four structures.
Compound C
Possible conformations (circle one):
Дет
Lab Data
The distance entered is out of the expected range.
Check your calculations and conversion factors.
Verify your distance. Will the gas cloud be closer to the cotton ball with HCI or NH3?
Did you report your data to the correct number of significant figures?
- X
Experimental Set-up
HCI-NH3
NH3-HCI
Longer Tube
Time elapsed (min)
5 (exact)
5 (exact)
Distance between cotton balls (cm)
24.30
24.40
Distance to cloud (cm)
9.70
14.16
Distance traveled by HCI (cm)
9.70
9.80
Distance traveled by NH3 (cm)
14.60
14.50
Diffusion rate of HCI (cm/hr)
116
118
Diffusion rate of NH3 (cm/hr)
175.2
175.2
How to measure distance and calculate rate
For the titration of a divalent metal ion (M2+) with EDTA, the stoichiometry of the reaction is typically:
1:1 (one mole of EDTA per mole of metal ion)
2:1 (two moles of EDTA per mole of metal ion)
1:2 (one mole of EDTA per two moles of metal ion)
None of the above
Chapter 19 Solutions
Chemistry: Structure and Properties Custom Edition for Rutgers University General Chemistry
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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