For each of the following processes, indicate whether thesigns of ΔS and ΔH are expected to be positive, negative,or about zero. (a) A solid sublimes. (b) The temperature ofa sample of Co(s) is lowered from 60 °C to 25 °C. (c) Ethylalcohol evaporates from a beaker. (d) A diatomic moleculedissociates into atoms. (e) A piece of charcoal is combustedto form CO2(g) and H2O(g).
For each of the following processes, indicate whether thesigns of ΔS and ΔH are expected to be positive, negative,or about zero. (a) A solid sublimes. (b) The temperature ofa sample of Co(s) is lowered from 60 °C to 25 °C. (c) Ethylalcohol evaporates from a beaker. (d) A diatomic moleculedissociates into atoms. (e) A piece of charcoal is combustedto form CO2(g) and H2O(g).
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter10: Entropy And The Second Law Of Thermodynamics
Section: Chapter Questions
Problem 10.80PAE
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For each of the following processes, indicate whether the
signs of ΔS and ΔH are expected to be positive, negative,
or about zero. (a) A solid sublimes. (b) The temperature of
a sample of Co(s) is lowered from 60 °C to 25 °C. (c) Ethyl
alcohol evaporates from a beaker. (d) A diatomic molecule
dissociates into atoms. (e) A piece of charcoal is combusted
to form CO2(g) and H2O(g).
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