ChE Thermodynamics Flashcards

1
Q

Which law is the basis for the manufacture of thermometer?

A

Zeroth Law of Thermodynamics (thermal equilibrium)

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2
Q

Who coined the Zeroth Law of Thermodynamics?

A

Ralph Howard Fowler

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3
Q

These properties depend on the current state of the system and not on how the system reaches that state

A

State functions

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4
Q

Other name for the first law of thermodynamics

A

Law of Conservation of Energy (energy can neither be created nor destroyed and can only be transformed in various forms)

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5
Q

Who coined the Law of Conservation of Energy?

A

Rudolf Julius Emmanuel Clausius

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6
Q

Examples of state functions

A

Enthalpy (H), Entropy (S), Temperature, Pressure, Internal Energy

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7
Q

Examples of path functions

A

Heat (Q) and Work (W)

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8
Q

Which of the following statement is correct?
A. The standard heat of formation of an element is negative.
B. Since dH = dU + dPV and can never be equal to dU
C. Q and W are state functions
D. Q + W is a state function

A

D.

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9
Q

Formula for internal energy (U)

A

U = Q + W

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10
Q

It is the energy needed to create the system

A

Internal Energy (U)

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11
Q

It is the total heat of the system

A

Enthalpy (H)

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12
Q

Formula for enthalpy

A

dH = dU + dPV

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13
Q

For constant volume (isochoric) process, heat (Q) is equal to?

A

Internal energy (U)

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14
Q

For constant pressure (isobaric) process, heat (Q) is equal to?

A

Enthalpy (H)

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15
Q

Formula for enthalpy (H) during isobaric processes

A

dH = integral of CpdT

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16
Q

Formula for internal energy (U) during isochoric processes

A

dU = integral of CvdT

17
Q

Formula for CV at constant volume process

A

Cv = (partial derivative of U)/(partial derivative of T)

18
Q

Equation which relates pressure, volume, and temperature of a gas is called

A

Equation of state

19
Q

The equation, PV=nRT is best obeyed by gases at

A

low pressure, high temp

20
Q

The compressibility factor of a gas is:
A) not a function of pressure
B) not a function of its nature
C) not a function of its temperature
D) Unity, as it followes PV=nRT

21
Q

For monoatomic gases, Cp/Cv is equal to?

22
Q

For diatomic gases, Cp/Cv is equal to?

23
Q

Cp and Cv formulas for monoatomic gases

A

Cp = 5R/2
Cv = 3R/2

24
Q

Cp and Cv formula for diatomic gases

A

Cp = 7R/2
Cv = 5R/2

25
What happens to the internal energy of a gas during an isothermal process?
Remains unchanged
26
In an adiabatic process
Heat transfer is zero
27
From PV^n, when n=0, the process is
Isobaric
28
From PV^n, when n=1, the process is
Isothermal
29
From PV^n, when n=sigma, the process is
Adiabatic
30
A solid is transformed into vapor without going through the liquid phase at?
Below the triple point, or at triple point
31
Formula for irreversible work when reversible work is positive
Wirrev= Wrev/efficiency
32
Formula for irreversible work when reversible work is negative
Wirrev= Wrev(efficiency)
33
Other formula for virial coefficient of state
PV/RT = (1+ B/V+ C/V^2)
34
Adiabatic Relations Page sa perry's
10-64
35
Actual work divided by the corresponding ideal work is known as ___ efficiency.
Turbine
36
Heat capacity is defined as C = dQ/dT, what is the difficulty about the relationship of C to Q which are supposedly state functions? A. It is a process-dependent quantity B. It indicates that small temp changes have smaller capacities C. It is not an intensive property D. It presents heat as energy in transit
A.
37
Which gives the most work we can get out of an adiabatic system?
Reversible expansion
38
What happens to delta U when work is done by the system during the adiabatic expansion of ideal gas?
Decreases
39
Formula for Tr and Pr
Tr = T/Tc Pr = P/Pc