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WorksheetsChapter 14 review
Total questions: 15
Worksheet time: 12mins
Which one of the following thermodynamic quantities is not a state function?
Gibbs free energy
enthalpy
entropy
work
A system suffers an increase in internal energy of 80 J and at the same time has 50 J of work done on i
+130 J
+30 J
-130 J
-30 J
All of the following have a standard heat of formation value of zero at 25oC and 1.0 atm except:
N2(g)
Fe(s)
Ne(g)
H(g)
Thermodynamics
ability to do work create heat
the study of energy
the study of heat flow
the study of chemical
Energy
the ability to do work
the energy available to do work
the measure of the disorder of a system
the thermal energy content of a system
Exergy
the energy available to do work
the thermal energy content of a system
the ability to do work
the measure of the disorder of a system
what are the three laws of thermodynamics
The energy in the universe is constant
Things get more disorganized over time in a system until everything is equal
You can’t reach absolute zero
You can reach absolute zero
Kinetic energy
(a)
as temperature increases, the entropy of the system
increases
decreases
three methods of heat transfer
conduction
kinetic energy
radiation
convection
Which one of the following is an expression of the van't Hoff equation?
ln K = - ΔHθ / RT + ΔSθ /R
ΔH(T2) = ΔH(T1) + ΔCp(T2 - T1)
ΔGθ = ΔHθ - TΔSθ
ΔU = q + w
Which one of the following statements describes a path function?
A property of a system that depends only on the current state of the system, not on the path the system took to reach that state
A property of a system that depends on the path taken between the initial and final states
The sum of kinetic and potential energy contained in a substance
The heat energy absorbed by a system at constant pressure
Which of the following is true for a steady flow system?
mass does not enter or leave the system
mass entering can be more or less than the mass leaving
mass entering = mass leaving
none of the mentioned
Which of the following statements is incorrect?
When solid and liquid iron are in equilibrium, ΔG = 0.
On going from solid copper to molten copper, ΔSo < 0.
When a solid dissolves in a solvent, ΔsolHo may be positive or negative.
For a phase change from liquid to vapour, Δvap H = ΔvapS × Tb where Tb = boiling point of the liquid.
Which statement is incorrect about entropy?
For a phase change, ΔS = 0.
The value of So for a compound or element depends on temperature.
The entropy of a system + surroundings increases during a spontaneous, irreversible process.
A pure, perfect crystal has zero entropy at 0 K.
