ME6301 ENGINEERING THERMODYNAMICS SHORT QUESTIONS AND ANSWERS - UNIT IV

ME 6301
ENGINEERING
THERMODYNAMICS
unit - iv
[FOR THIRD SEMESTER B.E MECHANICAL
ENGINEERING STUDENTS]
COMPILED BY
BIBIN.C
ASSISTANT PROFESSOR
DEPARTMENT OF MECHANICAL ENGINEERING
RMK COLLEGE OF ENGINEERING AND TECHNOLOGY
GUMMIDIPOONDI TALUK
TIRUVALLUR DIST

ME 6301 - ENGINEERING THERMODYNAMICS
UNIT IV - IDEAL AND REAL GASES AND THERMODYNAMIC RELATIONS
1. Define Ideal gas.
It is defined as a gas having no forces of intermolecular attraction. These gases will
follow the gas laws at all ranges of pressures and temperatures.
2. Define Real gas.
It is defined, as a gas having the forces of attraction between molecules tends to be
very small at reduced pressures and elevated temperatures.
3. State Boyle's law.
It states that volume of a given mass of a perfect gas varies inversely as the absolute
pressure when temperature is constant.
4. State Charle's law.
It states that if any gas is heated at constant pressure, its volume changes directly as
its absolute temperature.
5. What is equation of state?
The relation between the independent properties such as pressure, specific volume
and temperature for a pure substance is known as the equation of state.
6. Explain law of corresponding states.
If any two gases have equal values of reduced pressure and reduced temperature,
then they have same values of reduced volume.
7. What do you mean by reduced properties?
The ratios of pressure, temperature and specific volume of a real gas to the
corresponding critical values are called the reduced properties.
COMPILED BY BIBIN, AP/MECH, RMKCET Page 2

8. What is partial pressure?
The partial pressure of each constituent is that pressure which the gas would exert
if it occupied alone that volume occupied by the mixtures at the same temperature.
9. Define Dalton's law of partial pressure.
The total pressure exerted in a closed vessel containing a number of gases is equal
to the sum of the pressures of each gas and the volume of each gas equal to the volume of
the vessel.
10.Explain Dalton's law of partial pressure.
The pressure of a mixture of gases is equal to the sum of the partial pressures of the
constituents. The partial pressure of each constituent is that pressure which the gas would
expect if it occupied alone that volume occupied by the mixtures at the same temperatures.
m = m A+m B+m C+……. = ∑mi
mi = mass of the constituent.
P=P A+P B+P C+……. = ∑P i
P i - the partial pressure of a constituent.
11.What is compressibility factor?
The gas equation for an ideal gas is given by (PV/RT) = 1, for real gas (PV/RT) is not
equal to 1 (PV/RT) = Z for real gas is called the compressibility factor.
12.Explain the construction and give the use of generalized compressibility chart.
The general compressibility chart is plotted with Z versus P r for various values of
Tr . This is constructed by plotting the known data of one of mole gases and can be used
for any gas. This chart gives best results for the regions well removed from the critical
state for all gases.

13.State Avogardo's Law.
The number of moles of any gas is proportional to the volume of gas at a given
pressure and temperature.
14.What is Joule-Thomson coefficient?
The temperature behaviors of a fluid during a throttling (h=constant) process is
described by the Joule-Thomson coefficient defined as
µ =[δT/δP]n
15.How does the Vander Waal's equation differ from the ideal gas equation of state?
The ideal gas equation pV=mRT has two important assumptions,
i. There is little or no attraction between the molecules of the gas.
ii. That the volume occupied by the molecules themselves is negligibly small
compared to the volume of the gas. This equation holds good for low
pressure and high temperature ranges as the intermolecular attraction and
the volume of the molecules are not of much significance.
As the pressure increases, the inter molecular forces of attraction and
repulsion increases and the volume of the molecules are not negligible. The real gas
deviates considerably from the ideal gas equation [p+(a/V 2)](V-b) = RT
16.What are the assumptions made in Vanderwaal's equation of state?
i. There is no intermolecular force between particles.
ii. The volume of molecules is negligible in comparison with the gas.
17.Define coefficient of volume expansion.
The coefficient of volume expansion is defined as the change in volume with the
change in temperature per unit volume keeping the pressure constant. It is denoted byβ.

18.State Helmholtz function.
Helmholtz function is the property of a system and is given by subtracting the
product of absolute temperature (T) and entropy (S) from the internal energy (U).
Helmholtz function = U – TS
19.What are thermodynamic properties?
Thermodynamic properties are pressure (p), temperature (T), volume (V), internal
energy (U), enthalpy(H), entropy (S), Helmholtz function (α) and Gibbs function (g).
20.Define Molecular mass.
Molecular mass is defined as the ratio between total mass of the mixture to the total
number of moles available in the mixture.
21.Define isothermal compressibility.
Isothermal compressibility is defined as the change in volume with change in
pressure per unit volume keeping the temperature constant.

ME6301 ENGINEERING THERMODYNAMICS SHORT QUESTIONS AND ANSWERS - UNIT IV

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ME6301 ENGINEERING THERMODYNAMICS SHORT QUESTIONS AND ANSWERS - UNIT IV