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engineering
introduction to chemical engineering thermodynamics

Introduction To Chemical Engineering Thermodynamics 2nd Edition HALDER - Solutions

Excess property of a component can be schematically represented by(a) \(H^{\mathrm{E}}=H-H^{\text {id }}\)(b) \(H^{\mathrm{E}}=H^{\text {id }}-H\)(c) \(H^{\mathrm{E}}-H^{\mathrm{id}}=H\)(d) None of these.
"The fugacity of each component in an ideal solution is proportional to the mole fraction of that pure component in the solution." This is known as(a) Henry's law(b) Raoult's law(c) Lewis-Randall rule(d) Gibbs law.
The Lewis-Randall rule is applicable(a) At high pressures(b) At low pressures when the gas mixture behaves as an ideal solution(c) At low temperature(d) At low temperature and high pressure.
Raoult's law can be expressed as(a) \(\bar{P}_{i}=y_{i} P_{i}^{\text {sat }}\)(b) \(\bar{P}_{i}=y_{i}^{\text {sat }} P_{i}\)(c) \(P_{i}^{\text {sat }}=y_{i} \bar{P}_{i}\)(d) None of these.
Raoult's law is found to be quite satisfactory for a(a) Dilute solution(b) Ideal solution(c) Non-ideal solution(d) Perfect gas.
For an ideal solution, the enthalpy change of mixing \(\left(\Delta H_{\text {mix }}\right)\) is always given by(a) \(\Delta H_{\text {mix }}=1\)(c) \(\Delta H_{\text {mix }}=-1\)(b) \(\Delta H_{\text {mix }}=0\)(d) \(\Delta H_{\text {mix }}=\infty\).
Predict the correct form of the Gibbs-Duhem equation in terms of the activity coefficient:(a) \(x_{1} \frac{d \ln \gamma_{1}}{d x_{1}}=\left(1-x_{2}\right) \frac{d \ln \gamma_{2}}{d x_{2}}\)(b) \(\left(1-x_{1}\right) \frac{d \ln \gamma_{1}}{d x_{1}}=x_{2} \frac{d \ln \gamma_{2}}{d x_{2}}\)(c)
For a binary ideal solution, if \(x_{1}\) and \(x_{2}\) are the mole fractions of components 1 and 2 respectively, then(a) \(x_{1}+x_{2}=0\)(b) \(x_{1}+x_{2}=-1\)(c) \(x_{1}+x_{2}=1\)(d) \(x_{1}+x_{2}=\infty\).
In a binary ideal solution consisting of components \(\mathrm{A}\) and \(\mathrm{B}\)(a) Component A obeys Raoult's law and component B obeys Henry's law(b) Component A obeys Henry's law and component B obeys Raoult's law(c) Both the components obey Raoult's law(d) None of these.
Pick up the correct sentence out of the following:(a) Minimum boiling azeotropes may be formed if a solution exhibits very small positive deviation from ideal behaviour(b) Maximum boiling azeotropes may be formed if the solution exhibits very large positive deviation from ideal behaviour(c) Minimum
The criterion of phase equilibrium of a component is(a) \(d G_{T, P, V}=0\)(b) \(d G_{T, P}=1\)(c) \(d G_{T, P}=0\)(d) \(d A_{T, P}=0\).
The vapour-liquid equilibrium of a binary system can be better represented by(a) Temperature-composition \((T-X-Y)\) diagram(b) Pressure-composition \((P-X-Y)\) diagram(c) Pressure-temperature \((P-T)\) diagram(d) All of these.
The boiling point diagram of a binary mixture can be represented with the help of the(a) Temperature versus volume plot(b) Pressure versus volume plot(c) Pressure versus composition plot(d) Temperature versus composition plot.
The boiling point diagram of a binary solution is used to know how the equilibrium changes with(a) Pressure(b) Free energy(c) Temperature(d) Entropy.
The bubble point and dew point curves meet where the mixture turns into(a) Purely two components(b) Purely one component(c) Purely three components(d) None of these.
The term azeotrope means(a) Condensing without changing(b) Boiling without changing(c) Both (a) and (b)(d) Neither (a) nor (b).
Excess Gibbs free energy models are used to determine the value of the(a) Isothermal compressibility(c) Coefficient of volume expansion(b) Activity coefficient(d) Gibbs' free energy.
For the determination of the activity coefficient for the system comprising relatively simple and preferably non-polar liquids, we generally use the(a) Wohl's equation(b) Margules equation(c) Van Laar equation(d) Wilson equation.
The disadvantage(s) of the Wilson equation over the van Laar equation is/are that(a) It can not be applied for the systems in which \(\gamma\) shows maxima or minima(b) It is not suitable for the systems exhibiting limited miscibility(c) Neither (a) nor (b) (d) Both (a) and (b).
The advantage(s) of the UNIQUAC equation is/are that(a) It is suitable for solutions having small as well as large molecules(b) The equation is simple as it consists of only two adjustable parameters(c) It is also applicable to a good number of non-polar solutions such as aldehydes and ketones(d)
Bubble point is defined as the point at which(a) The first bubble of vapour is formed upon heating a liquid consisting of two or more components at a given pressure(b) The first drop of liquid (condensate) is formed upon cooling the vapour at a given pressure(c) A saturation point is reached(d) A
For checking the thermodynamic consistency of VLE data(a) A test is usually performed on the basis of the Gibbs-Duhem equation in terms of the activity coefficients(b) The data can be obtained from the pressure-temperature-mole fractions \((P-T-x-y)\) diagram(c) A test is usually performed on the
For a ternary system having a homogeneous single phase, the degree(s) of freedom will be(a) 3(b) 4(c) 2(d) 1 .
The depression of freezing point is defined as the difference between(a) The freezing points of the pure solvent and the solution containing the volatile solute(b) The melting points of the pure solvent and the solution containing the non-volatile solute(c) The freezing points of the pure solvent
The magnitude of the osmotic pressure depends on the(a) Temperature(b) Gibbs' free energy(c) Nature of the semi-permeable membrane(d) Entropy.
The reaction coordinate(a) Is a one-dimensional coordinate(b) Indicates the progress of a chemical reaction along a pathway(c) Is a geometric parameter that changes during the conversion of one or more molecular entities(d) All of these.
A chemical reaction must proceed in the direction of(a) Increasing Gibbs free energy(c) Constant Gibbs free energy(b) Decreasing Gibbs free energy(d) None of these.
The equilibrium criterion of a chemical reaction can be expressed as(a) \((d G)_{T, P}=1\)(b) \((d G)_{T, P}=-1\)(c) \((d G)_{T, P}=0\)(d) \((d G)_{T, P}=\infty\).
For a chemically reacting system, the relation between Gibbs' free energy change and equilibrium constant is given by(a) \(K=e^{-\frac{R T}{\Delta \dot{G}}}\)(b) \(K=e^{-\frac{\Delta \dot{\circ}}{R T}}\)(c) \(K=e^{\frac{\Delta \mathscr{G}}{R T}}\)(d) \(K=e^{\frac{\Delta \dot{G} R}{T}}\).
Heterogeneous reaction is defined as the reaction which requires(a) At least one phase to proceed(b) At least two phases to proceed(c) One initiator to take place(d) One negative catalyst to take place.
The phase rule for a chemically reacting system was formulated by(a) Gibbs-Duhem(b) Gibbs(c) Arrhenius(d) Van't Hoff.
The phase rule for a chemically reacting system differs from the same for a non-reacting system in terms of(a) The number of phases(b) The number of independent reactions(c) The number of components(d) None of these.
A fuel cell is an electrochemical energy conversion device in which(a) The chemical energy of a fuel is converted directly into electrical energy(b) The electrical energy of a fuel is converted directly into chemical energy(c) The chemical energy of a fuel is converted directly into mechanical
The fuel cell(a) Produces power at low cost at considerable periods(b) Requires quite extensive maintenance(c) Has harmful by-products(d) None of these.
The criterion for equilibrium for a chemically reacting system(a) Is independent of the laws of thermodynamics(b) Is obtained from the first and second laws of thermodynamics(c) Can not be obtained unless the fundamental relation is known(d) None of these.
A process is said to be feasible if(a) \(\Delta G>0\)(b) \(\Delta G
For a chemically reacting system at constant temperature and pressure, the criterion for equilibrium can be expressed as(a) \(\Sigma \mu_{i} d n_{i}=0\)(b) \(\Sigma n_{i} d \mu_{i}1\).
For an ideal gas the change in Gibbs' free energy at constant temperature is given by(a) \(R d \ln T\)(b) \(R T d \ln V\)(c) \(R T d \ln P\)(d) None of these.
The activity of component \(i\) can be written as(a) \(a_{i}=\frac{f_{i}^{0}}{f_{i}}\)(b) \(a_{i}=\frac{f_{i}}{f_{i}^{0}}\)(c) \(a_{i}=\ln \left(\frac{f_{i}}{f_{i}^{0}}\right)\)(d) \(a_{i}=\ln \left(f_{i}-f_{i}^{0}\right)\).
The influence of temperature on the equilibrium constant of a chemical reaction can be obtained from(a) \(\left(\frac{\partial \ln K}{\partial T}\right)=-\frac{\Delta \dot{H}}{T^{2}}\)(b) \(\ln \frac{K_{2}}{K_{1}}=\frac{\Delta \stackrel{\circ}{H}}{R}\left(\frac{1}{T_{2}}-\frac{1}{T_{1}}\right)\)(c)
In the steady flow energy equation, which of the following remains constant?(a) Entropy(b) Pressure(c) Enthalpy(d) Total energy.
For the reaction \(\mathrm{CO}(\mathrm{g})+2 \mathrm{H}_{2}(\mathrm{~g}) \rightarrow \mathrm{CH}_{3} \mathrm{OH}(\mathrm{g})\), with increase in pressure the degree of conversion(a) Decreases(b) Increases(c) Remains constant(d) None of these.
Methanol can be produced by the following reaction\[ \mathrm{CO}(\mathrm{g})+2 \mathrm{H}_{2}(\mathrm{~g}) \rightarrow \mathrm{CH}_{3} \mathrm{OH}(\mathrm{g}) \]If some inert gas is added to the reaction mixture, then the degree of conversion(a) Decreases(b) Does not change(c) Increases(d) None of
Hydrogen gas is produced according to the reaction\[ \mathrm{CH}_{4}(\mathrm{~g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \rightarrow \mathrm{CO}(\mathrm{g})+3 \mathrm{H}_{2}(\mathrm{~g}) \]With increase in pressure the degree of conversion(a) Decreases(b) Increases(c) Remains constant(d) None of
For the reaction \(\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \rightarrow 2 \mathrm{NH}_{3}(\mathrm{~g})\), maximum conversion can be achieved if the reaction takes place at(a) Low pressure and high temperature(b) Low temperature and high pressure(c) Low pressure and low
Given that the standard free energy of formation at \(298 \mathrm{~K}\) for \(\mathrm{NH}_{3}\) is \(-16.750 \mathrm{~kJ} / \mathrm{mol}\), the standard Gibbs' free energy change for the ammonia synthesis reaction \(\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}\) (g) \(\rightarrow 2
The chemical potential of component \(i\) in a solution mixture can be expressed as(a) \(\mu_{i}=R T \ln G_{i}^{0}+a_{i}\)(c) \(\mu_{i}=R T \ln G_{i}^{0}-a_{i}\)(b) \(\mu_{i}=R T \ln a_{i}+G_{i}^{0}\)(d) \(\mu_{i}+R T \ln G_{i}^{0}=a_{i}\).
The chemical potential of a pure substance is equal to the(a) Specific Gibbs' free energy(b) Molar entropy(c) The Gibbs' free energy(d) Molar Gibbs' free energy.
In an ideal gas mixture consisting of components \(A\) and \(B\), the partial pressure of component \(A\) is equal to(a) \(p_{\mathrm{A}}=\frac{n_{\mathrm{A}}-n_{\mathrm{B}}}{N}\)(b) \(p_{\mathrm{A}}=\frac{N}{n_{\mathrm{A}}+n_{\mathrm{B}}}\)(c)
In an ideal gas mixture consisting of components \(A\) and \(B\), the mole fraction of component \(A\) is equal to(a) \(n_{\mathrm{A}}=\frac{p_{\mathrm{A}}+p_{\mathrm{B}}}{P}\)(b) \(n_{\mathrm{A}}=\frac{p_{\mathrm{A}}-p_{\mathrm{B}}}{P}\)(c)
In an absorption refrigeration system, the heat energy \(Q_{1}\) is supplied at temperature \(T_{1}\) while the system absorbs heat energy \(Q_{3}\) from a cold space at temperature \(T_{3}\). If the ambient temperature is \(T_{2}\), then the COP of the refrigerator (ignoring the negligible amount
For any pure substance, the difference between \(C_{P}\) and \(C_{V}\) can be expressed in terms of the isothermal compressibility \(\alpha\) and volume expansivity \(\beta\) as(a) \(C_{P}-C_{V}=\frac{T V \beta}{\alpha^{2}}\)(b) \(C_{P}-C_{V}=\frac{T V \beta^{2}}{\alpha}\)(c) \(C_{P}-C_{V}=\frac{T
The availability of a system(a) Depends upon the conditions of the system only(b) Is independent of the conditions of the surroundings(c) Does not depend upon the conditions of the system(d) Depends upon the conditions of the system and the surroundings.
The sudden bursting of a cycle tyre is an(a) Isothermal process(b) Isochoric process(c) Isobaric process(d) Adiabatic process.
Changes of state such as melting, vaporization and freezing are(a) Adiabatic processes(b) Isothermal processes(c) Isochoric processes(d) Isobaric processes.
A process during which a system returns to its initial state through a number of different processes is called a/an(a) Adiabatic process(b) Isothermal process(c) Cyclic process(d) Iso-volumetric process.
When the heat capacity ratio is 1.67 , then the ideal gas is(a) Diatomic(b) Monatomic(c) Triatomic(d) None of these.
According to the phase rule, the triple point of a pure substance is(a) Invariant(b) Univariant(c) Divariant(d) None of these.
The internal energy of an element at \(1 \mathrm{~atm}\) and \(25^{\circ} \mathrm{C}\) is(a) \(0 \mathrm{kcal} / \mathrm{kmol}\)(b) \(25 \mathrm{kcal} / \mathrm{kmol}\)(c) \(273 \mathrm{kcal} / \mathrm{kmol}\)(d) None of these.
Which of the following changes during phase transition?(a) Pressure(b) Volume(c) Temperature(d) All of these.
The acentric factor for all materials is always(a) 0(b) 1(c) \(1\).
For a binary system comprising two miscible non-reacting components in vapour-liquid equilibrium forming an azeotrope, the number of degrees of freedom is(a) 0(b) 1(c) 2(d) 3 .
Melting of ice is an example of(a) Adiabatic process(b) Isothermal process(c) Isochoric process(d) Isobaric process.
The equation of state for a certain gas is given by \(P(V-(\mathrm{b})=R T\), where \(b\) is a positive constant. The Joule-Thomson coefficient of this gas would be(a) + ve(b) - ve(c) Zero(d) None of these.
As time passes, the entropy of the universe(a) Decreases(b) Increases(c) Remains constant(d) Can not be predicted.
A \(4 \mathrm{~m}^{3}\) rigid tank contains nitrogen gas at \(400 \mathrm{kPa}\) and \(350 \mathrm{~K}\). Now heat is transferred to the nitrogen in the tank and the pressure of nitrogen rises to \(700 \mathrm{kPa}\). The work done during the process is(a) \(900 \mathrm{~kJ}\)(b) \(500
Air-conditioning machine operates on the principle of(a) Second law of thermodynamics(b) Zeroth law of thermodynamics(c) First law of thermodynamics(d) Third law of thermodynamics
The phase rule is coined by(a) Gibbs(b) Helmholtz(c) Joule(d) van der Waals
The temperature and pressure of air are \(30^{\circ} \mathrm{C}\) and \(1 \mathrm{~atm}\) respectively. The mass of air behaving ideally contained in a room of size \(5 \mathrm{~m} \times 5 \mathrm{~m} \times 5 \mathrm{~m}\) is(a) \(234.2 \mathrm{~kg}\)(b) \(144.9 \mathrm{~kg}\)(c) \(204.6
For an ideal gas, the slope of the pressure-volume curve at a given point will be(a) Steeper for an adiabatic process than for an isothermal process(b) Steeper for an isothermal process than for an adiabatic process(c) Identical for both the processes(d) None of the above
The distribution coefficient (k) depends upon(a) Temperature only(b) Pressure only(c) Temperature and pressure only(d) Temperature, pressure and concentration
For an ideal gas mixture undergoing a reversible gaseous phase chemical reaction, the equilibrium constant(a) Increases with pressure(c) Is not dependent of pressure(b) Decreases with pressure(d) None of these
The ratio of the intake volume to the displacement volume in a single-stage compressor is called(a) Isentropic efficiency(b) Theoretical volumetric efficiency(c) Actual volumetric efficiency(d) Swept volumetric efficiency
A car tyre of volume \(0.057 \mathrm{~m}^{3}\) is inflated to \(300 \mathrm{kPa}\) and \(300 \mathrm{~K}\). After driving the car for 10 hours, the pressure in the tyre increases to \(330 \mathrm{kPa}\). Assume air is an ideal gas and \(C_{V}\) for air is \(21 \mathrm{~J} /
The shaft work done by the fluid in a reversible flow process in which there are no changes in the kinetic, potential and surface energies, is given by(a) \(W_{\text {shaft }}=\int_{1}^{2} P d V\)(b) \(W_{\text {shaft }}=\int_{2}^{1} P d V\)(c) \(W_{\text {shaft }}=\int_{2}^{1} V d P\)(d)
The change in entropy for an ideal gas undergoing a thermodynamic process is(a) \(S_{2}-S_{1}=-R \ln \frac{V_{1}}{V_{2}}\)(b) \(S_{2}-S_{1}=-R \ln \frac{P_{1}}{P_{2}}\)(c) \(S_{2}-S_{1}=R \ln \frac{V_{1}}{V_{2}}\)(d) \(\quad S_{2}-S_{1}=R \ln \frac{P_{1}}{P_{2}}\)
A flat balloon is inflated by filling it with helium from a tank of compressed helium. The final volume of the balloon is \(6 \mathrm{~m}^{3}\). The barometer reads \(100 \mathrm{kPa}\). Consider the tank, the balloon, and the connecting pipe as a system. The work done against the atmosphere is(a)
The degree of freedom of a system comprising a gaseous mixture of \(\mathrm{H}_{2}\) and \(\mathrm{NH}_{3}\) will be(a) 1(c) 3(b) 2(d) 0
An inventor claims to have developed an engine that takes in \(100 \mathrm{MJ}\) of heat at \(400 \mathrm{~K}\), rejects \(40 \mathrm{MJ}\) of heat at \(200 \mathrm{~K}\), and delivers \(15 \mathrm{kWh}\) of mechanical work. The claim of the inventor is(a) True(b) False(c) Invalid(d) None of these
When the temperature of an ideal gas is increased from \(27^{\circ} \mathrm{C}\) to \(927{ }^{\circ} \mathrm{C}\), the kinetic energy will be(a) Same(b) Twice(c) Eight times(d) Four times
The value of \(\Delta W=\int_{1}^{2} P d V\) of an ideal gas in a reversible isothermal process is(a) 0(b) \(\frac{P_{1} V_{1}-P_{2} V_{2}}{\gamma-1}\)(c) \(P_{1} V_{1} \ln \frac{V_{2}}{V_{1}}\)(d) \(P_{1}\left(V_{2}-V_{1}\right)\)
Compressibility factor for a given vapour or gas can be represented by(a) \(Z=1+B^{\prime} P+C^{\prime} P^{2}+D^{\prime} P^{3}+\cdots\)(b) \(Z=1+\frac{B}{V}+\frac{C}{V^{2}}+\frac{D}{V^{3}}+\cdots\)(c) Either(a) or (b)(d) None of these
\(n_{1}\) moles of an ideal monoatomic gas at temperature \(T_{1}\) and pressure \(P\) are in one compartment of an, insulated container. In an adjoining compartment, separated by an insulating partition three are \(n_{2}\) moles of another ideal monoatomic gas at temperature \(T_{2}\) and pressure
The work done in reversible polytropic steady flow processes is given by(a) \(\frac{P_{1} V_{1}-P_{2} V_{2}}{n-1}\)(b) \(\frac{n\left(P_{1} V_{1}-P_{2} V_{2}\right)}{n-1}\)(c) \(n\left(P_{1} V_{1}-P_{2} V_{2}\right)\)(d) \(\frac{n\left(P_{1} V_{1}-P_{2} V_{2}\right)}{n+1}\)
For the slope of an isothermal and adiabatic curves through a point on \(P-V\) diagram of an ideal gas, the relation is(a) Slope of an isothermal curve \(=\) slope of an adiabatic curve(b) Slope of an isothermal curve \(=\gamma\) (slope of an adiabatic curve)(c) Slope of an adiabatic curve
On a Mollier chart, the slope of the curve representing a reversible isobaric process is equal to(a) \(T-\beta\)(b) \(T+\frac{1}{\beta}\)(c) \(T\)(d) \(\beta T-1\)
On a Mollier diagram, the slope of the curve representing a reversible isothermal process is equal to(a) \(T-\beta\)(b) \(T-\frac{1}{\beta}\)(c) \(T\)(d) \(T+\frac{1}{\beta}\)
Critical pressure ratio for the flow of gases through a converging nozzle is given by(a) \(\left(\frac{2}{\gamma+1}\right)^{\gamma / \gamma-1}\)(b) \(\left(\frac{1}{\gamma+1}\right)^{\gamma / \gamma-1}\)(c) \(\left(\frac{2 \gamma}{\gamma+1}\right)^{\gamma / \gamma-1}\)(d) None of these
A system, consisting of \(2 \mathrm{~mol}\) of \(\mathrm{N}_{2}, 5 \mathrm{~mol}\) of \(\mathrm{H}_{2}\) and \(2 \mathrm{~mol}\) of \(\mathrm{NH}_{3}\) initially, is undergoing the following reaction:\[ \mathrm{N}_{2}+3 \mathrm{H}_{2} \rightarrow 2 \mathrm{NH}_{3} \]Derive the expression for the
The study of thermodynamics enables us to understand(a) Whether the transformation of energy is feasible or not(b) To what extent the transformation will take place(c) In which direction the transformation will take place(d) All of these.
The following reaction takes place in a system consisting of \(3 \mathrm{~mol} \mathrm{CH}_{4}, 5 \mathrm{~mol} \mathrm{H}_{2} \mathrm{O}\), \(1 \mathrm{~mol} \mathrm{CO}\) and \(4 \mathrm{~mol} \mathrm{H}_{2}\) initially:\[ \mathrm{CH}_{4}(\mathrm{~g})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{g})
A thermodynamic system(a) Is a definite quantity of matter(b) Is surrounded by a boundary(c) Can exchange energy with its surroundings(d) All of these.
Develop the expressions for the mole fractions of reacting species as functions of the reaction coordinate for a system initially containing \(3 \mathrm{~mol} \mathrm{H}_{2} \mathrm{~S}\) and \(5 \mathrm{~mol} \mathrm{O}_{2}\) undergoing the following reaction:\[ 2 \mathrm{H}_{2}
A system is said to be in thermodynamic equilibrium if its(a) Temperature remains unchanged(b) Pressure remains unchanged(c) Chemical potential remains unchanged(d) Temperature, pressure and chemical potential remain unchanged.
A system initially containing \(3 \mathrm{~mol} \mathrm{CO}_{2}, 5 \mathrm{~mol} \mathrm{H}_{2}\) and \(1 \mathrm{~mol} \mathrm{H}_{2} \mathrm{O}\) is undergoing the following reactions:\[ \begin{aligned} \mathrm{CO}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) & \rightarrow \mathrm{CH}_{3}
A process in which pressure remains constant is called(a) Isochoric process(b) Isobaric process(c) Isothermal process(d) Adiabatic process.
A system is initially charged with \(4 \mathrm{~mol}\) ethylene and \(3 \mathrm{~mol}\) oxygen, and the following reaction occurs between the species:\[ \begin{aligned} \mathrm{C}_{2} \mathrm{H}_{4}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) & \rightarrow 2\left[\left(\mathrm{CH}_{2}\right)
The variables of a system which are proportional to the size of the system are called(a) Extensive variables(b) Mass variables(c) Intensive variables(d) Thermodynamic variables.
Calculate the standard Gibbs free energy change and the equilibrium constant at 1 bar and \(298.15 \mathrm{~K}\) for the ammonia synthesis reaction\[ \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(\mathrm{g})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{~g}) \rightarrow \mathrm{CH}_{3}
A system in which mass as well as energy can not be exchanged with the surroundings is called(a) Open system(b) Closed system(c) Isolated system(d) None of these.

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