Gases tend to behave non-ideally at low temperatures and high pressures. The deviation from ideal behaviour can be explained by considering two types of corrections. They are volume correction and pressure correction. Select incorrect statement(s) :
A
A closed system with all adiabatic boundaries must be an isolated system
B
Total heat exchange in a cyclic process may be zero
C
Entropy of a closed system is maximum at equilibrium
D
Molar Gibb's Energy is an extensive property
Text Solution
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The correct Answer is:
A, C, D
(a) In isolated system no change possible (b) `DeltaU=q+w=0implies q=-w` w may be zero so q may be zero. (c ) Entropy of a closed system is not maximum at equilibrium. (d) Intensive properties.
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Gases tend to behave non-ideally at low temperatures and high pressures. The deviation from ideal behaviour can be explained by considering two types of corrections. They are volume correction and pressure correction. Following represents equation of state for a mules of real gas [P + (n^2a)/(V^2)][V-nb] = nRT .Select incorrect statement for a real gas
Gases tend to behave non-ideally at low temperatures and high pressures. The deviation from ideal behaviour can be explained by considering two types of corrections. They are volume correction and pressure correction. Which assumption of kinetic theory is not followed when a real gas shows non-ideal behaviour ?
(A): A gas behaves as an ideal gas at high temperature and low pressure. (R): Helium behaves as an ideal gas under all conditions.
Consider following statements : (A): The gas whose critical temperature is above room temperature can be liquified by applying sufficient pressure to the gas. (B): The gas whose critical temperature is below room temperature can be liquified by the temperature below T_c . Select correct statement
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Ideal gas equation is represented as PV=nRT . Gases present in the universe were found ideal n the Boyle's temperature range only. The compressibility factor for an ideal gas, Z= (PV)/(nRT) . The main cause to show deviations were due to wrong assumptions made bout forces of attractions (which becomes significant at high pressure). olume occupied by molecules V, in PV = nRT, is supposed to be volume of as or, the volume of container in which gas is placed by assuming that aseous molecules do not have appreciable volume. Actual volume of the as is that volume in which each molecule of a gas can move freely. If olume occupied by gaseous molecule is not negligible, then the term V hould be replaced by the ideal volume which is available for free motion of ach molecule of gas. Similarly for n moles of gas V_("actual") = V-nb The excluded volume can be calculated by considering bimolecular collisions. The excluded volume is the volume occupied by the sphere of 2r for each pair of molecule. Thus, excluded volume for one pair of molecules = 4/3 pi (2r)^3 = (4 xx 8 pi r^3)/3 The excluded volume for 1 molecule = 2/3 xx 8 pi r^3 = 4 xx (4/3 pi r^3) = 4V The excluded volume for N molecules = 4NV = b (where N is Avogadro's No.) The compressibility factor for N_2 at -50^@C and 800 atm pressure is 1.95. Number of moles of N_2 required to fill a balloon of 100 L capacity is :
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