Part I
Thermodynamics is a chemical process that entails transformations in temperature, changes in energy, and the correlation that exists between work and heat. Thermodynamics is vital in different unit processes as it helps determine both enthalpy and equilibrium data for design used in distillation, absorption evaporators, and condensers column units. It can also be used in various units involving heat change. Besides, thermodynamics give relevant information on effects of heat, maxim conversion and other variables.(a) In chemical processes, equilibrium refers to the condition when the two products and reactants are available in constant concentrations over a period of time. The properties of a chemical system therefore remain unchanged.
Chemical equilibrium can also e described as the state in which the content of the units in a chemical system are same in the whole system and a reaction does not occur in the chemical system.
(b)Vapor-liquid equilibrium for non-ideal system refers to a state in which a perfect mixture exists both in vapor and liquid phases. In thermal equilibrium there is no clear transfer of mass in the phases. Vapor- liquid mixture is separated using both gravity and heat. The mixture is added in the system, which is then converted to a vacuum using a vacuum pump. The vapor condenses and mixes with the liquid. It is then passed to the chamber where boiling takes place. The mixture is separated due to the difference in boiling points. XXXXX XXX a XXXXXX XXXXXXX XXXXX than the other XXXXXXXXXX in XXX mixture. The XXXXXXXXXX that XXX volatile in XXX mixture therefore XXXXXXXXX.
X. (a) TX = XXXX, XC = XXXX, W = 2.XXX
Efficiency = 1 - = 1-
Efficiency = 0.XXXXX
QX =
XH = X.XXXXX
XC = QH – X = X.028 – X.5
QC= X.XXXXX
= X.005556 kJ/K
(b) Heat XXXXXXXX is XXX heat required to XXXXXXXX a XXXXX quantity of a XXXXXXXXX XX one Kelvin. XXXXX heat capacity XX a gas is XXX heat XXXXXX to XXXXX the temperature of XXX mole XX the gas through XXX
Kelvin.
XXXX XXXXXXX: XX = nC x XX
At XXXXXXXX XXXXXX XX
XX = nCX x dT
XXXX XXX XXX XX XXXXXXXXXXXXXX: dQ = dE - dW
XXXX volume XX XXXXXXXX: dQ = dE
Hence, XX = dE = nCX x XX =
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nR dT ,
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Comparing, XX get, XXX a XXXXXXXXX ideal gas: XX
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= X
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(diatomic:
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CX
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=
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R)
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XXXXX dQ = XX, XX XXXXXXXX XXXXXX, XX = n CV x XX.
XX Constant XXXXXXXX XP
dQ = XXX x XX
From XXX Law XX Thermodynamics: XX = XX - dW
When XXXXXXXX is constant: dQ = XX
XXXXX, XX = XX = nCP x XX =
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XX dT ,
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Comparing, we get, for a monatomic XXXXX XXX: CV
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= R
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(XXXXXXXX:
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CX
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=
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X)
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Since dQ = XX, at constant volume, dE = n XX x dT.
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