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• For a reversible process: ∆Suniv = 0. • For a spontaneous process (i.e. irreversible): ∆Suniv > 0. • Note: the second law states that the entropy of the universe must increase in a spontaneous process. It is possible for the entropy of a system to decrease as long as the entropy of the surroundings increases.
process. This means ∆H - T∆S < 0 for a spontaneous process • Two factors determine spontaneity: ∆H and T∆S • Reaction more likely to be spontaneous if ∆H < 0 (exothermic) T large and ∆S large and positive • However, none of these factors is required if the other factors are larger (e.g., water freezes even
the process is directed towards the equilibrium: infinitesimal action cannot stop the process. • Non-spontaneous process: improbable. Non-spontaneous process may become spontaneous only by redefining a universe, e.g. including in a universe something that can change equilibrium. • Reversible process: the system is at equilibrium: infinitesimal
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A spontaneous process is a process that happens without intervention in a given set of conditions. In a spontaneous reaction, the formation of products is more favorable. Spontaneity is determined by the overall change in Gibb’s free energy (ΔG), i.e. energy available to do work. A reaction is
Aug 14, 2020 · A process that is spontaneous in one direction under a particular set of conditions is nonspontaneous in the reverse direction. At room temperature and typical atmospheric pressure, for example, ice will spontaneously melt, but water will not spontaneously freeze. The spontaneity of a process is not correlated to the speed of the process. A ...
For a reversible process: ∆S univ = 0. For a spontaneous process (i.e. irreversible): ∆S univ > 0. C. Molecular Interpretation of Entropy • A gas is less ordered than a liquid which is less ordered than a solid. • Any process which increases the number of gas molecules leads to an increase in entropy. • When NO(g) reacts with O
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Nils Walter: Chem 260 The spontaneity of chemical reactions Atkins, Chapter 4 Reaction: 2 H 2 (g) + O 2 (g) → 2 H 2 O(l) ∆ r S Univ = ∆ r S Sys + ∆ r S Surr
