Thermodynamics
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<p><strong>3. The enthalpies of all elements in their standard states are: </strong></p>
<p><strong>(i)</strong> Unity <strong> </strong></p>
<p><strong>(ii) </strong>Zero</p>
<p><strong>(iii)</strong> < 0 <strong> </strong></p>
<p><strong>(iv)</strong> Different for each element</p>
<p><strong>2. For the process to occur under adiabatic conditions, the correct condition is:</strong></p>
<p><strong>(i) </strong>?T= 0 <strong> </strong></p>
<p><strong>(ii) </strong>?p = 0</p>
<p><strong>(iii) </strong>q = 0 <strong> </strong></p>
<p><strong>(iv) </strong>w = 0 </p>
1. Choose the correct answer:
A thermodynamic state junction is a quantity
(i) Used to determine heat changes
(ii) Whose value is independent of path
(iii) Used to determine pressure volume work
(iv) Whose value depends on temperature only.
1. Choose the correct answer:
A thermodynamic state junction is a quantity
(i) Used to determine heat changes
(ii) Whose value is independent of path
(iii) Used to determine pressure volume work
(iv) Whose value depends on temperature only.
1. (ii) whose value is independent of path
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<p><strong>Choose the correct answer: </strong></p>
<p><strong>A thermodynamic state junction is a quantity</strong></p>
<p><strong>(i) </strong>Used to determine heat changes</p>
<p><strong>(ii)</strong> Whose value is independent of path</p>
<p><strong>(iii)</strong> Used to determine pressure volume work</p>
<p><strong>(iv) </strong>Whose value depends on temperature only.</p>
Although heat is a path function but heat absorbed by the system under certain specific conditions is independent of path. What are those conditions? Explain.
Although heat is a path function but heat absorbed by the system under certain specific conditions is independent of path. What are those conditions? Explain.
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 vo
Upvote Predict the change in internal energy for an isolated system at constant volume.
Predict the change in internal energy for an isolated system at constant volume.
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
Upvote Which quantity out of ∆rG and ∆rGᶱ will be zero at equilibrium?
Which quantity out of ∆rG and ∆rGᶱ will be zero at equilibrium?
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&nbs
Upvote The molar enthalpy of vapourisation of acetone is less than that of water. Why?
The molar enthalpy of vapourisation of acetone is less than that of water. Why?
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.
Upvote Identify the state functions and path functions out of the following : enthalpy, entropy, heat, temperature, work, free energy.
Identify the state functions and path functions out of the following : enthalpy, entropy, heat, temperature, work, free energy.
This is a Short Answer Type Questions as classified in NCERT Exemplar
State functions: Enthalpy, entropy, temperature, free energy Path functions: Heat, work.
Upvote The standard molar entropy of H2O (l) is 70 J K–1 mol–1. Will the standard molar entropy of H2O(s) be more, or less than 70 J K–1 mol–1?
The standard molar entropy of H2O (l) is 70 J K–1 mol–1. Will the standard molar entropy of H2O(s) be more, or less than 70 J K–1 mol–1?
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 l
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