Spontaneity table

In chemistry, a spontaneity table is table showing a summarized view of how variations in the quantities ΔH, ΔS, and T can combine to determine or yield different spontaneity outcomes chemical reactions.

Overview
A few comparative versions of these spontaneity tables are shown below, in chronological order.

Ebbing spontaneity table (1990)LeMay spontaneity table (1996)
Darrell Ebbing's 1990 spontaneity table. [1] A 1996 Eugene LeMay spontaneity table. [2]
Raghavan spontaneity table (1997)

Raghavan spontaneity table (1997). [7]


Delta G tableBrown spontaneity table (2003)
Raymond Change's 1998 spontaneity table. [3]Theodore Brown's 2003 spontaneity table. [4]
Whitten spotaneity table (2007)





Reger spontaneity table 2009

Kenneth Whitten's 2007 spontaneity table. [5]
A 2009 Daniel Reger spontaneity table. [6]


American chemist Darrell Ebbing's 1990 spontaneity table is asterisked to note that the terms ‘low temperature’ and ‘high temperature’ are relative, to the effect that for certain reactions, high temperature could mean room temperature. [1] We note that room temperature is the temperature at which the majority of human chemical reactions occur, albeit with seasonal fluctuation influence.

American chemist Raymond Change’s 1998 table notes that when both ΔH and ΔS are negative that the reverse reaction becomes spontaneous at high temperatures, which loosely finds corroboration with the finding that "divorce season", which begins January 02, corresponds to the point in time at which day light hours begin to increase, and hence the point in time when the system begins to be heated more and more each day.

In 2014, Jason Kahn, in his TEDx talk “Connecting Thermodynamics to Everything” (ΡΊ), gave the following spontaneity table:

Spontaneity table
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References
1. Ebbing, Darrell D. (1990). General Chemistry (pg. 733). Houghton Mifflin Co.
2. LeMay, Eugene, Robblee, Karen M, Baell, Herbert, and Brower, Douglas C. (1996). Chemistry: Connections to Our Changing World (pg. 762). Prentice Hall.
3. Chang, Raymond. (1998). Chemistry (pg. 740). McGraw-Hill.
4. Brown, Theodore L., LeMay, H. Eugene, Burstein, Bruce, and Burdge, Julia R. (2003). Chemistry (pg. 760). Prentice Hall.
5. Whitten, Kenneth W. (2007). Chemistry (pg. 587). Cengage Learning.
6. Reger, Daniel L. (2009). Chemistry: Principles and Practice (pg. 753). Cengage Learning.
7. Raghavan, P.S. (1997). Concepts and Problems in Physical Chemistry (pg. 269). Discovery Publishing House.

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