Thermodynamics
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3 months agoContributor-Level 10
This is a Short Answer Type Questions as classified in NCERT Exemplar
At constant volume
q = ΔU + (-w)
-w = pΔ q = AU + pΔV
ΔV = 0 (at constant volume)
Hence, qv = ΔU + 0 = ΔU= change in internal energy at constant pressure, qp = AU + pΔV
Since ΔU + pΔV=ΔH
=> qp = ΔH change in enthalpy
Hence, at constant volume and at constant pressure, heat change is a state function because it is equal to ΔU and ΔH respectively which are state functions.
New answer posted
3 months agoContributor-Level 10
This is a Short Answer Type Questions as classified in NCERT Exemplar
For an isolated system w = 0, q = 0
Since ΔU= q + w = 0 + 0 = 0, ΔU= 0
New answer posted
3 months agoContributor-Level 10
This is a Short Answer Type Questions as classified in NCERT Exemplar
Gibbs energy for a reaction in which all reactants and products are in standard state. ΔrG° is related to the equilibrium constant of the reaction as follows
ΔrG = ArG° + RT In K
At equilibrium, 0 = ΔrG° + RT InA– ( {ΔrG = 0) or ΔrG° =-RT lnK
ΔrG° = 0 when K= 1
For all other values of K, ArG° will be non-zero.
New answer posted
3 months agoContributor-Level 10
This is a Short Answer Type Questions as classified in NCERT Exemplar
Molar enthalpy of vaporization is more for water due to hydrogen bonding between water molecules.
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3 months agoContributor-Level 10
This is a Short Answer Type Questions as classified in NCERT Exemplar
State functions: Enthalpy, entropy, temperature, free energy Path functions: Heat, work.
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3 months agoContributor-Level 10
This is a Short Answer Type Questions as classified in NCERT Exemplar
The standard molar entropy of H20 (1) is 70 J K-1 mol-1. The solid form of H20 is ice. In ice, molecules of H20 are less random than in liquid water. Thus, molar entropy of H20 (s) < molar entropy of H20 (1). The standard molar entropy of H20 (s) is less than 70 J K-1 mol-1.
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