An ice cube at 0 C melts when placed inside a room at 22 C (295 K). Based on the concepts of enthalpy, entropy, and Gibbs free energy, which of the following best explains why the process is thermodynamically favorable? Melting ice releases energy, AH < 0, and AS < O because the motion of the H20 molecules decreases as it transitions from solid to liquid. At a temperature higher than 0 C (273 K). the term TAS is smaller than AH", resulting in a thermodynamically favorable process with AG < 0. Melting ice releases energy, AH' < 0, and AS' > 0 because the motion of the H20 molecules increases as it transitions from solid to liquid. At a temperature higher than 0 C (273 K), в the term TAS" is greater than AH", resulting in a thermodynamically favorable process with AG > 0. Melting ice requires energy, AH" >0, and AS < O because the motion of the H,O molecules decreases as it transitions from solid to liquid. At a temperature higher than 0"C (273 K), the term TAS is smaller than AH", resulting in a thermodynamically favorable process with AG > 0. Melting ice requires energy, AH' >0, and AS' >0 because the motion of the H20 molecules increases as it transitions from solid to liquid. At a temperature higher than 0 C (273 K), D the term TAS" is greater than AH", resulting in a thermodynamically favorable process with AG" < 0.
An ice cube at 0 C melts when placed inside a room at 22 C (295 K). Based on the concepts of enthalpy, entropy, and Gibbs free energy, which of the following best explains why the process is thermodynamically favorable? Melting ice releases energy, AH < 0, and AS < O because the motion of the H20 molecules decreases as it transitions from solid to liquid. At a temperature higher than 0 C (273 K). the term TAS is smaller than AH", resulting in a thermodynamically favorable process with AG < 0. Melting ice releases energy, AH' < 0, and AS' > 0 because the motion of the H20 molecules increases as it transitions from solid to liquid. At a temperature higher than 0 C (273 K), в the term TAS" is greater than AH", resulting in a thermodynamically favorable process with AG > 0. Melting ice requires energy, AH" >0, and AS < O because the motion of the H,O molecules decreases as it transitions from solid to liquid. At a temperature higher than 0"C (273 K), the term TAS is smaller than AH", resulting in a thermodynamically favorable process with AG > 0. Melting ice requires energy, AH' >0, and AS' >0 because the motion of the H20 molecules increases as it transitions from solid to liquid. At a temperature higher than 0 C (273 K), D the term TAS" is greater than AH", resulting in a thermodynamically favorable process with AG" < 0.
Chemistry for Engineering Students
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ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
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Chapter10: Entropy And The Second Law Of Thermodynamics
Section: Chapter Questions
Problem 10.50PAE: For the reaction NO(g)+NO2(g)N2O3(g) , use tabulated thermodynamic data to calculate H and S. Then...
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Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
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Question 22D
An ice cube at 0°C melts when placed inside a room at 22 C (295 K). Based on the concepts of enthalpy, entropy, and Gibbs free energy, which of the following best explains why the process is
thermodynamically favorable?
Melting ice releases energy, AH < 0, and AS <O because the motion of the H,O molecules decreases as it transitions from solid to liquid. At a temperature higher than 0°C (273 K),
A
the term TAS is smaller than AH", resulting in a thermodynamically favorable process with AG" < 0.
Melting ice releases energy, AH < 0, and AS> 0 because the motion of the H,0 molecules increases as it transitions from solid to liquid. At a temperature higher than 0 C (273 K),
B
the term TAS is greater than AH, resulting in a thermodynamically favorable process with AG > 0.
Melting ice requires energy, AH >0, and AS < 0 because the motion of the H,O molecules decreases as it transitions from solid to liquid. At a temperature higher than 0 C (273 K),
the term TAS is smaller than AH, resulting in a thermodynamically favorable process with AG > 0.
Melting ice requires energy, AH>0, and AS >0 because the motion of the H,0 molecules increases as it transitions from solid to liquid. At a temperature higher than 0 C (273 K),
D
the term TAS is greater than AH, resulting in a thermodynamically favorable process with AG" < 0.
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