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engineering
introduction to chemical engineering thermodynamics

Introduction To Chemical Engineering Thermodynamics 2nd Edition HALDER - Solutions

The degrees of freedom at the triple point will be(a) 0(c) 2(b) 1(d) 3 .
The free energy change for a chemical reaction is given by(a) \(R T \ln K\)(b) \(-R T \ln K\)(c) \(-R \ln K\)(d) \(T \ln K\).
The ratio of the adiabatic compressibility to the isothermal compressibility is(a) 1(b) \(>1\)(c) \(>>1\)(d) \(
The efficiency of a Carnot engine working between the temperatures \(T_{1}\) and \(T_{2}\) \(\left(T_{1}
1 ton of refrigeration capacity is equivalent to the heat removal rate of(a) \(50 \mathrm{kcal} / \mathrm{hr}\)(b) \(200 \mathrm{kcal} / \mathrm{hr}\)(c) \(200 \mathrm{BTU} / \mathrm{min}\)(d) \(200 \mathrm{BTU} / \mathrm{d}\).
In an ideal solution, the activity of a component is equal to its(a) Fugacity(b) Mole fraction(c) Vapour pressure(d) Partial pressure.
The efficiency of an Otto engine compared to that of a diesel engine for the same compression ratio will be(a) More(b) Less(c) Equal(d) Data insufficient.
Gibbs' free energy of a pure fluid approaches at constant temperature(a) Infinity(b) Minus infinity(c) Zero(d) None of these.
The value of the activity coefficient for an ideal solution is(a) 1(b) 0(c) Equal to Henry's law constant(d) Equal to vapour pressure.
The phase rule for a system can be written as(a) \(F=C-P-1\)(b) \(F=C-P+1\)(c) \(F=C+P+2\)(d) \(F=C-P+2\)where \(C=\) Number of components\(P=\) Number of phases\(F=\) Degrees of freedom.
"The rate at which a substance reacts is proportional to its active mass and the rate of a chemical reaction is proportional to the product of the active masses of the reacting substances." This is the(a) Lewis-Randall rule(b) Statement of the Van't Hoff equation(c) Le Chatelier's principle(d) None
The first law of thermodynamics is concerned with the(a) Direction of energy transfer(b) Reversible processes only(c) Irreversible processes only(d) None of these.
The point at which solid, liquid, and gas phases co-exist is known as the(a) Freezing point(b) Triple point(c) Boiling point(d) None of these.
For an ideal gas, slope of the pressure-volume curve at a given point will be(a) Steeper for an isothermal process than for an adiabatic process(b) Steeper for an adiabatic process than for an isothermal process(c) Identical for both the processes(d) Of opposite sign.
Which of the following is not affected by temperature?(a) Fugacity(b) Activity co-efficient(c) Free energy(d) All of these.
Fugacity and pressure are numerically not equal for a gas(a) At low temperature and high pressure(b) At standard state(c) Both(a) and (b)(d) In an ideal state.
Gibbs' free energy of a pure fluid approaches — as the pressure tends to zero at constant temperature(a) Infinity(b) Minus infinity(c) Zero(d) None of these.
For an ideal solution, the value of the activity coefficient is(a) 0(b) 1(c) \(1\).
A good halogenated refrigerant should have(a) High thermal conductivity(b) Low freezing point(c) Zero ozone depletion potential(d) All of these.
In the reaction represented by \(2 \mathrm{SO}_{2}+\mathrm{O}_{2}=2 \mathrm{SO}_{3}, \Delta \mathrm{H}=-42 \mathrm{kcal}\), the forward reaction will be favoured by(a) Low temperature(b) High pressure (c) Both (a) and (b)(d) Neither (a) nor (b).
In a homogeneous solution, the fugacity of a component depends upon the(a) Pressure(b) Composition(c) Temperature(d) All of these.
Clausius-Clayperon equation is applicable to(a) Solid-vapour(b) Solid-liquid(c) Liquid-vapour(d) All of these.
The reaction \(A(\mathrm{l}) \rightarrow R(\mathrm{~g})\) is allowed to reach equilibrium condition in an autoclave. At equilibrium there are two phases - one a pure liquid phase of \(A\) and the other a vapour phase of \(A, R\) and \(S\). Initially \(A\) alone is present. The number of degrees of
The equilibrium constant for the reaction \(\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{NH}_{3}\) is 0.1084 . Under the same conditions, the equilibrium constant for the reaction \((1 / 2) \mathrm{N}_{2}(\mathrm{~g})+(3 / 2) \mathrm{H}_{2}(\mathrm{~g})\)
In the ammonia synthesis reaction \(\mathrm{N}_{2}+3 \mathrm{H}_{2}=2 \mathrm{NH}_{3}+22.4 \mathrm{kcal}\), the formation of \(\mathrm{NH}_{3}\) will be favoured by(a) High temperature(b) Low pressure(c) Low temperature only(d) Both low temperature and high pressure.
The internal energy of an ideal gas depends on(a) Temperature, specific heat and volume(b) Temperature and specific heat(c) Temperature, specific heat and pressure(d) Pressure, volume and temperature.
For steady flow, the first law of thermodynamics(a) Is concerned with heat interaction(b) Is an energy balance for a specified mass of fluid(c) Accounts for all energy entering and leaving a control volume(d) None of these.
A control volume refers to(a) A selected region in space for the analysis of a problem(b) An isolated system(c) A homogeneous system(d) A fixed mass.
At constant temperature, the volume of a given mass of a gas is inversely proportional to the pressure. This is known as(a) Avogadro's law(b) Charles' law(c) Boyle's law(d) none of these.
The major limitation of the first law of thermodynamics is that it does not consider(a) The direction of change(b) The extent of change(c) Both (a) and (b)(d) Neither (a) nor (b).
\(C_{P}=C_{V}\) for a fluid which is(a) Incompressible(b) Compressible(c) Of very low volume expansivity(d) None of these.
The entropy change of a system is zero in a/an(a) Reversible process(b) Isochoric process(c) Isobaric process(d) Reversible adiabatic process.
For \(n\) moles of an ideal gas, \(C_{P}-C_{V}\) is(a) \(n R\)(c) \(R^{n}\)(b) \(R\)(d) \(n^{R}\).
Fugacity has the same dimension as(a) Temperature(b) Pressure(c) Activity coefficient(d) Work done.
At the triple point of water, the number of degrees of freedom is(a) One(b) Two(c) Zero(d) Three.
\(C_{P}=C_{V}\) when(a) \(\left(\frac{\partial V}{\partial T}\right)_{P}=0\)(b) \(\left(\frac{\partial V}{\partial P}\right)_{T}=0\)(c) \(\left(\frac{\partial P}{\partial T}\right)_{V}=0\)(d) None of these.
"If the two bodies are in thermal equilibrium with a third body, they are also in thermal equilibrium with each other." This is known as the(a) First law of thermodynamics(b) Second law of thermodynamics(c) Third law of thermodynamics(d) Zeroth law of thermodynamics.
The three-parameter corresponding state is concerned with(a) Temperature, pressure and volume(b) Reduced temperature, reduced pressure and reduced volume(c) Critical temperature, critical pressure and critical volume(d) Critical temperature, critical pressure and acentric factor.
The inversion point of a gas is defined as the temperature at which the Joule-Thomson coefficient \((\mu)\) is equal to(a) 0(b) 1(c) -1(d) \(\infty\).
State which one of the following is correct:(a) \(d G=-S d T+V d P\)(b) \(d U=T d S+P d V\)(c) \(d H=T d S-V d P\)(d) \(d A=-S d T+P d V\).
Enthalpy can be expressed as(a) \(H=U-P V\)(b) \(H-U=P V\)(c) \(H=A-T S\)(d) \(H-A=T S\).
The mathematical expression of the first law of thermodynamics is(a) \(d Q=d U+P d V\)(b) \(d Q=d U-d W\)(c) \(d U=d Q+P d V\)(d) \(d W=d Q+d U\).
Isothermal compressibility of a substance is given by(a) \(\alpha=\frac{1}{V}\left(\frac{\partial V}{\partial P}\right)_{T}\)(b) \(\alpha=-\frac{1}{V}\left(\frac{\partial V}{\partial P}\right)_{T}\)(c) \(\alpha=-\frac{1}{V}\left(\frac{\partial P}{\partial V}\right)_{T}\)(d) None of these.
Volume expansivity of a pure substance is given by(a) \(\beta=-\frac{1}{V}\left(\frac{\partial V}{\partial T}\right)_{P}\)(b) \(\beta=\frac{1}{V}\left(\frac{\partial V}{\partial T}\right)_{P}\)(c) \(\beta=V\left(\frac{\partial V}{\partial T}\right)_{P}\)(d) \(\beta=\frac{1}{V}\left(\frac{\partial
In the vapour absorption refrigeration system, the compression section is replaced by an assembly of(a) Absorber, heat exchanger and generator(b) Absorber, liquid pump, heat exchanger and generator(c) Absorber, liquid pump and heat exchanger(d) Absorber, liquid pump and generator.
The combined law of thermodynamics is represented by(a) \(d U=T d S-P d V\)(b) \(d U=T d S+P d V\)(c) \(d U=d Q+P d V\)(d) None of these.
The Clausius inequality is expressed mathematically as(a) \(\oint \frac{d Q}{T}
The efficiency of a refrigerating machine operating between two thermal reservoirs depends upon the(a) Nature of the working fluid only(b) Two reservoir temperatures only(c) Mass of the working fluid(d) Both pressure and temperature of the working fluid.
Joule-Thomson expansion is an(a) Isothermal process(b) Isochoric process(c) Isenthalpic process(d) Isentropic process.
The work done due to isothermal expansion is(a) \(W=n R T \ln \frac{P_{1}}{P_{2}}\)(b) \(W=n R T \ln \frac{V_{2}}{V_{1}}\)(c) \(W=n R T \ln \frac{V_{1}}{V_{2}}\)(d) Both (a) and (b).
\(C_{V}\) for an ideal gas(a) Is independent of temperature only(b) Is independent of pressure only(c) Is independent of volume only(d) Is independent of both pressure and volume.
The highest temperature and pressure above which a liquid can not exist is known as the(a) Triple point(b) Critical point(c) Freezing point(d) Boiling point.
The equation which relates pressure, volume and temperature is known as the(a) Clausius-Clapeyron equation(b) Kammerlingh-Onnes equation(c) Equation of state(d) Maxwell's equation.
An irreversible process always leads to \(\mathrm{a} / \mathrm{an}\)(a) Decrease in entropy(b) Increase in entropy(c) Constancy in entropy(d) None of these.
Reduced temperature of a pure substance is the ratio of its(a) Critical temperature to temperature(b) Critical temperature to saturated temperature(c) Saturated temperature to critical temperature(d) Temperature to critical temperature.
The deviation from ideal gas behaviour can be accounted for by a correction factor called the(a) Acentric factor(b) Solubility factor(c) Compressibility factor(d) None of these.
For an ideal gas(a) \(\left(\frac{\partial U}{\partial V}\right)_{T}=1\)(b) \(\left(\frac{\partial U}{\partial V}\right)_{T}=0\)(c) \(\left(\frac{\partial U}{\partial V}\right)_{T}=-1\)(d) None of these.
The expansion of a gas takes place against zero pressure. This phenomenon is called(a) Isothermal expansion(b) Joule-Thomson expansion(c) Isentropic expansion(d) Free expansion.
The Joule-Thomson coefficient \(\mu\) of a gas can be mathematically represented by(a) \(\mu=\left(\frac{\partial T}{\partial P}\right)_{H}\)(b) \(\mu=\left(\frac{\partial V}{\partial P}\right)_{H}\)(c) \(\mu=\left(\frac{\partial P}{\partial T}\right)_{H}\)(d) \(\mu=\left(\frac{\partial P}{\partial
The standard state assigned for a thermodynamic property is(a) \(1 \mathrm{~atm}\) and \(273 \mathrm{~K}\)(b) \(1 \mathrm{~atm}\) and \(298 \mathrm{~K}\)(c) \(1 \mathrm{~atm}\) and \(300 \mathrm{~K}\)(d) none of these.
Entropy is a measure of the(a) Randomness of a system(b) Orderly configuration of molecules(c) Non-randomness of a system(d) None of these.
For a constant pressure process(a) \(d H=C_{V} d T\)(b) \(d H=\int C_{V} d T\)(c) \(d H=C_{P} d T\)(d) \(d H=d Q_{P}\).
For a constant volume process(a) \(d U=C_{V} d T\)(b) \(\Delta U=\int C_{V} d T\)(c) \(d U=T d S-P d V\)(d) \(d U=C_{P} d T\).
According to Charles' law(a) \(V \propto P\) while \(T=\) constant(b) \(V \propto 1 / P\) while \(T=\) constant(c) \(V \propto 1 / T\) while \(P=\) constant(d) \(V \propto T\) while \(P=\) constant.
According to Boyle's law for gases(a) \(V \propto T\) while \(P=\) constant(b) \(V \propto 1 / P\) while \(T=\) constant(c) \(V \propto 1 / T\) while \(P=\) constant(d) \(V \propto P\) while \(T=\) constant.
The heat capacity at constant pressure \(\left(C_{P}\right)\) is defined as(a) \(C_{P}=\left(\frac{\partial U}{\partial T}\right)_{P}\)(b) \(C_{P}=\left(\frac{\partial Q}{\partial T}\right)_{P}\)(c) \(C_{P}=\left(\frac{\partial H}{\partial T}\right)_{P}\)(d) \(C_{P}=\left(\frac{\partial W}{\partial
The heat capacity at constant volume \(\left(C_{V}\right)\) is defined as(a) \(C_{V}=\left(\frac{\partial S}{\partial T}\right)_{V}\)(b) \(C_{V}=\left(\frac{\partial Q}{\partial T}\right)_{V}\)(c) \(C_{V}=\left(\frac{\partial H}{\partial T}\right)_{V}\)(d) \(C_{V}=\left(\frac{\partial U}{\partial
For an exothermic process, heat is(a) Absorbed by the system(b) Liberated from the system(c) Accumulated in the system(d) None of these.
For an endothermic reaction(a) \(\Delta H=+\mathrm{ve}\)(b) \(\Delta H=-\mathrm{ve}\)(c) \(\Delta H=\infty\)(d) \(\Delta H=0\).
"For a given chemical process, the net heat change will be the same whether the process occurs in one or in several stages." This is known as(a) Kirchoff's law(b) Hess's law(c) Laplace's law(d) Lavoisier's law.
The standard heat of reaction is expressed as(a) \(\Delta H_{\text {Reaction }}^{0}=\Sigma \Delta H_{\text {Reactants }}^{0}-\Sigma \Delta H_{\text {Products }}^{0}\)(b) \(\Delta H_{\text {Reaction }}^{0}=\Sigma \Delta H_{\text {Products }}^{0}-\Sigma \Delta H_{\text {Reactants }}^{0}\)(c) \(\Delta
The heat of combustion of a gas is generally determined with the help of the(a) Bomb calorimeter(b) Dean and Stark apparatus(c) Optical pyrometer(d) Orsat analyser.
If a reaction proceeds without loss or gain of heat and if all the products remain together in a single mass or stream of materials, these products will assume a definite temperature known as the(a) Adiabatic flame temperature(b) Adiabatic reaction temperature(c) Flash point(d) Both (a) and (b).
The work function or Helmholtz free energy is defined as(a) \(H=U-T S\)(b) \(H=U-T S\)(c) \(A=U-T S\)(d) \(W=U-T S\).
Gibbs' free energy is defined as(a) \(G=U-T S\)(b) \(G=H-T S\)(c) \(G=H-T S\)(d) None of these.
The internal energy of an ideal gas is a function of(a) Temperature only(b) Pressure only(c) Volume only(d) All of these.
The commercial refrigerating machine follows the principle of the(a) Carnot cycle(b) Reversed Carnot cycle(c) Stirling cycle(d) None of these.
The condition for spontaneity of a chemical reaction is(a) \(\Delta G_{T, P}0\)(d) None of these.
The equilibrium constant of a chemical reaction is influenced by the(a) Pressure(b) Temperature(c) Initial concentration of the reacting substance(d) None of these.
In refrigeration cycle, heat is(a) Abstracted from the lower temperature region and discarded to the higher one(b) Absorbed from the higher temperature region and discarded to the lower one(c) Both (a) and (b)(d) Neither (a) nor (b).
The chemical potential of a component is given by(a) \(\mu_{i}=\left(\frac{\partial G}{\partial n_{i}}\right)_{T, P}\)(b) \(\mu_{i}=\left(\frac{\partial A}{\partial n_{i}}\right)_{T, P, n_{i}}\)(c) \(\mu_{i}=\left(\frac{\partial G}{\partial n_{i}}\right)_{T, P, n_{i}}\)(d)
The van Laar equation is useful in determining the activity co-efficient of \(a / a n\)(a) Azeotropic mixture(b) Ternary solution(c) Binary solution(d) None of these.
The thermodynamic property relations are helpful in determining the(a) Measurable thermodynamic properties(b) Immeasurable thermodynamic properties(c) Change in free energy of the process(d) Reference properties only.
The influence of temperature on chemical equilibrium is substantiated by the(a) Arrhenius equation(b) Le Chatelier's principle(c) Van't Hoff equation(d) None of these.
The entropy change for a reversible process is always(a) 0(b) \(>0\)(c) \(
The Claude gas liquefaction process employs the \( \qquad \) for producing cooling effect(a) Isenthalpic expansion of gas(b) Isentropic expansion of gas(c) Isochoric expansion of gas(d) Isobaric expansion of gas.
At constant pressure and temperature, Gibbs' free energy due to mixing is always(a) 0(b) \(\infty\)(c) + ve(d) - ve.
The phase change process at varied equilibrium pressure and temperature is concerned with(a) Maxwell's equation(b) Gibbs-Helmholtz equation(c) Clapeyron equation(d) Gibbs-Duhem equation.
The free energy for a spontaneous process(a) Decreases(b) Increases(c) Is zero(d) None of these.
Free energy change at equilibrium is(a) Zero(b) Positive(c) Negative(d) Indeterminate.
For an irreversible process, the free energy is(a) - ve(b) + ve(c) 0(d) None of these.
The equilibrium constant of a chemical reaction does not depend upon(a) The temperature at equilibrium(b) The pressure at equilibrium(c) Neither(a) nor (b)(d) Both(a) and (b).
For a system prepared by partially decomposing \(\mathrm{CaCO}_{3}\) into an evacuated space, the number of degrees of freedom is(a) 2(b) 0(c) 1(d) 3 .
The number of degrees of freedom for a system prepared by partially decomposing \(\mathrm{NH}_{4} \mathrm{Cl}\) into an evacuated space is(a) 0(b) 1(c) 2(d) 3 .
For a system of two miscible non-reacting species which exists as an azeotrope in vapour-liquid equilibrium, the number of degrees of freedom is(a) 2(b) 0(c) 3(d) 1 .
The number of degrees of freedom for a system consisting of the gases \(\mathrm{CO}, \mathrm{CO}_{2}, \mathrm{H}_{2}\), \(\mathrm{H}_{2} \mathrm{O}\) and \(\mathrm{CH}_{4}\) in chemical equilibrium is(a) 0(b) 1(c) 3(d) 4 .
For the reaction \(2 \mathrm{SO}_{2}+\mathrm{O}_{2} \Leftrightarrow 2 \mathrm{SO}_{3}, \Delta H=-42 \mathrm{kcal}\), the forward reaction will be favoured by(a) Low temperature(b) High pressure(c) Both (a) and (b)(d) Neither (a) nor (b).
The efficiency of a Carnot engine working between \(500 \mathrm{~K}\) and \(200 \mathrm{~K}\) is(a) \(80 \%\)(b) \(75 \%\)(c) \(60 \%\)(d) \(70 \%\).
Pressure, volume, temperature and entropy are(a) Energy properties(b) Derived properties(c) Reference properties(d) None of these.
Work functions and free energy functions are(a) Derived properties(c) Reference properties(b) Energy properties(d) None of these.

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