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Thermodynamics An Interactive Approach 1st edition Subrata Bhattacharjee - Solutions

For a mixture of saturated vapor and saturated liquid of R-134a at 100 kPa, use tabulated properties or the PC system state TESTcalc to show that the chemical potentials of the two phases are equal.
Show that an equilibrium mixture of saturated vapor and saturated liquid of water at 100oC satisfies the criterion for phase equilibrium.
Consider a liquid-vapor mixture of ammonia and water in equilibrium at 15oC. If the molar composition of the liquid phase is 50% NH3 and 50% H2O, determine the composition of the vapor phase of this mixture.
A two-phase mixture of ammonia and water is in equilibrium at 40oC. If the molar composition of the vapor phase is 98% NH3 and 2% H2O, determine the composition of the liquid phase of this mixture.
Repeat 14-1-9 [BOS] for water at 100oC. Problem 14-1-9 A two-phase liquid-vapor mixture of R-134a is in equilibrium at 22oC. Show that the specific Gibbs functions of the saturated liquid and saturated vapor are equal.
For the reaction A + B ↔ C + D, Δg-o is calculated to be 0 at 500 K. Starting with a mixture of 1 kmol of A and 1 kmol of B, (a) Evaluate what percent of the mixture is converted to products at equilibrium at 500 kPa, 500 K. (b) What would be the answer if the pressure (p) were 1000 kPa?
For the dissociation of nitrogen tetraoxide described in problem 14-3-9 [BBO] , there is a 77.7% increase in volume when equilibrium is reached at 50oC, 125 kPa. Determine the value of the equilibrium constant (K).
A chamber contains a mixture of CO2, CO and O2 is in equilibrium at a specified temperature and pressure. How will (a) Increasing the temperature (T) at constant pressure and (b) Increasing the pressure (p) at constant temperature affect the number of moles of CO? (Enter 1 if increases, 2 if
Determine the change in the Gibbs function Δg-o at 25oC, in kJ/kmol, for the reaction CH4(g) + 2O2 ↔ CO2 + 2H2O(g) using enthalpy of formation and absolute entropy data.
Calculate the equilibrium constant (K) for CO2 ↔ CO + 1/2O2 at (a) 500 K and (b) 1000 K.
One kmol of CO2 is heated at a constant pressure of 100 kPa to 3000 K. (a) Calculate the equilibrium composition of CO2 and use the IGE system state TESTcalc to verify your answers. (b) Use the n-IG system state TESTcalc and calculate the Gibbs function of the mixture (1-x)CO2 + xCO + (x/2)O2 at
Calculate the equilibrium constant (K) for the water-gas reaction CO + H2O(g) ↔ CO2 + H2 at (a) 298 K and (b) 1000 K.
Determine the equilibrium constant (K) for the reaction H2 + 1/2O2 ↔ H2O at (a) 298 K and (b) 2500 K.
Determine the equilibrium constant (K) for the reaction CH4 + 2O2 ↔ CO2 + 2H2O at25oC.
Determine the equilibrium constant (K) for the dissociation process CO2 ↔ CO + 1/2O2 at (a) 298 K and (b) 2000 K.
For the chemical reaction CO2 + H2 ↔ CO + H2O, the equilibrium value of the degree of reaction (forward completion fraction) at 1200 K is 0.56. Determine the equilibrium constant and the change in Gibbs function.
For an elementary step A + B ↔ C + D, Δg - o is tabulated as 22.819 at 298 K, 0 at 1000 K, and -229.724 MJ/kmol at 3000 K. Starting with a mixture of 1 kmol of A and 1 kmol of B, evaluate what percent of the mixture is converted to products at equilibrium at (a) 298 K, (b) 1000 K, and (c) 3000
Determine the temperature at which 2% of diatomic oxygen (O2) dissociates into monatomic oxygen (O) at a pressure of 3 atm.
Oxygen (O2) is heated to 3000 K at a constant pressure of 5 atm. Determine the percentage of O2 that will dissociate into O during this process.
H2O(g) dissociates into an equilibrium mixture at 3000 K and 100 kPa. Assume the equilibrium mixture consists of H2(g), H2O, O2, and OH, determine the equilibrium composition of (a) H2O, (b) OH (in kmols).
Nitrogen (N2) is heated to 3000 K at a constant pressure of 5 atm. (a) Determine the percentage of N2 that will dissociate into N during this process. What-if Scenario: What would the answer be if the conditions were (b) 5 atm, 5000 K and (c) 0.1 atm, 5000 K?
Carbon dioxide (CO2) is heated to 3200 K at a constant pressure of 2 atm. Determine the percentage of CO2 that will dissociate into CO and O2 during the process.
Consider the dissociation of 1 kmol of A2 through the elementary step A2 ↔ 2A. If ε stands for the degree of dissociation (fraction of 2 by volume that is dissociated), the overall reaction can be represented by A2 ↔ (1-ε)A2 + 2εA. At 500 K and 100 kPa, the equilibrium constant is calculated
One kmol of carbon dioxide (CO2) is heated from 300 K to 4000 K at a constant pressure of 1 atm. Use the IGE system state TESTcalc, set up the reactants as 1 kmol of CO2 and select CO2, CO, and O2 as the possible products. Now calculate a series of equilibrium products states (in the state panel,
A mixture of 1 kmol of CO and 2 kmol of O2 is heated to 2000 K at a pressure of 2 atm. Determine the equilibrium composition of (a) O2, (b) CO2 (in kmols) assuming the mixture consists of CO2, CO and O2.
A mixture of 1 kmol of CO2, 1/2 kmol of O2 and 1/2 kmol of N2 is heated to 2900 K at a pressure of 1 atm. Determine the equilibrium composition of (a) CO2, (b) O2 assuming the mixture consists of CO2, CO, O2 and N2.
One kmol of carbon monoxide, CO, reacts with 1 kmol of oxygen, O2, to form an equilibrium mixture of CO2, CO and O2 at 2800 K. Determine the equilibrium composition of CO2 at (a) 1 atm, (b) 5 atm.
Evaluate Δg-o at 298 K for the reaction H2 + (1/2)O2 ↔ H2O using (a) Fundamental definition using formation enthalpy (h-o f) and entropy (s-o) values, and (b) Using formation Gibbs function from Table G-1.
One kmol of carbon monoxide (CO), reacts with theoretical amount of air to form an equilibrium mixture of CO2, CO, O2 and N2 at 2200 K and 1 atm. Determine the equilibrium composition of (a) CO, (b) CO2.
A mixture of 2 kmol of N2, 1 kmol of O2 and 0.1 kmol of Ar is heated to 2500 K at a constant pressure of 10 atm. Assuming the equilibrium mixture consists of N2, O2, Ar and NO, determine the equilibrium composition of (a) O2, (b) N2 (in kmols).
A chamber initially contains a gaseous mixture consisting of 4 kmol of CO2, 8 kmol of CO and 2 kmol of H2. Assume an equilibrium mixture formed consists of CO2, CO, H2O, H2 and O2 at 2600 K and 100 kPa, determine the equilibrium composition of (a) CO2, (b) CO (in kmols).
Butane (C4H10) burns inside a vessel with 50% excess air to form an equilibrium mixture at 1400 K and 1 MPa. The equilibrium mixture is composed of CO2, O2, N2, H2O(g), NO2, and NO. Determine the balanced reaction equation, use K = 8.4 × 10 - 10 for this reaction.
Methane (CH4) reacts with 125% of theoretical air inside a chamber to form an equilibrium mixture consisting of CO2, CO, H2O(g), H2, and N2 at 1200 K, 100 kPa. Determine the equilibrium composition of (a) CO2, (b) H2O (in kmols).
Octane (C8H18) reacts with 110% of theoretical air inside a chamber to form an equilibrium mixture consists of CO2, CO, H2O(g), H2, and N2 at 1650 K, 100 kPa. Determine the composition of the equilibrium mixture.
Starting with n0 kmol of NH3, which dissociates according to NH3 ↔ (1/2)N2 + (3/2)H2, evaluate an expression for K in terms of the degree of dissociation ε and pressure p.
Determine the mole fraction of sodium that ionizes according to the reaction Na ↔ Na+ + e- at 2300 K and 0.5 atm (use K = 0.688 for this reaction).
Determine the percent ionization of cesium that ionizes according to the reaction Ce ↔ Ce+ + e- at 2000 K and 1 atm (use K = 15.63 for this reaction).
Determine The pressure if the ionization of Ar is 80% complete according to the reaction Ar ↔ Ar+ + e- at 10,000 K (use K = 4.2 × 10-4 for this reaction).
Evaluate (a) Δh-o, (b) Δg-o, and (c) lnK at 298 K for the reaction CO + 1/2O2 ↔ CO2 at 1 atm.
One kmol of H2O is heated to 3000 K at a pressure of 1 atm. Determine the equilibrium composition of H2O (in kmols) assuming that only H2O , OH, O2 and O are present.
A mixture of 2 kmol of CO2 and 1 kmol of O2 is heated to 3200 K at a pressure of 5 atm. Determine the equilibrium composition of (a) CO, (b) CO2 (in kmols) assuming that only CO2, CO, O2 and O are present.
Air (21% O2, 79% N2) is heated to 2800 K at a pressure of 1 atm. Determine the equilibrium composition, assuming that only O2, N2, O and NO are present. Can the presence of NO in the equilibrium mixture be neglected?
The equilibrium constant for dissociation of N2O4 is 0.664 and 0.141 at 318 K and 298 K respectively. Calculate the average heat of reaction within this temperature range.
At an average temperature of 2000 K, the slope of the graph of log K against 1/T for the dissociation of water vapor (into hydrogen and oxygen) is found to be - 13000. (a) Determine the heat of dissociation. (b) Is this an exothermic reaction?
Potassium is ionized according to the equation K ↔ K+ + e-. The values of equilibrium constants at 3000 K and 3500 K are measured to be 8.33 × 10-6 and 1.33 × 10-4 respectively. Determine the average heat of reaction in MJ/kmol.
The equilibrium constant for the reaction SO3 †” SO2 + O has the following values:Determine the average heat of dissociation using graphical method.
1 kmol of Carbon at 25oC, 0.1 MPa reacts with 2.5 kmol of oxygen at 25oC, 0.1 MPa form an equilibrium mixture of CO2, CO and O2 at 3000 K, 0.1 MPa. Determine The amount of CO2 present in the products mixture and
A mixture of CO2, CO and O2 is in equilibrium at a specified temperature and pressure. Now the pressure is tripled, (a) Will the equilibrium constant K change? (b) Will the number of moles of CO2, CO and O2 change? How? (Enter 1 if increases, 2 if decreases, and 3 if no change)
Suppose the equilibrium constant of the dissociation reaction H2 = 2H at 2000 K and 1 atm is K1. Express the equilibrium constants of the following reactions at 2000 K in terms of K1: (a) H2 ↔ 2H at 4 atm, (b) 2H ↔ H2 at 1 atm, (c) 2H2 ↔ 4H at 1 atm, (d) H2 + 2N2 ↔ 2H + 2N2 at 2 atm and (e)
A mixture of NO, O2 and N2 is in equilibrium at a specified temperature and pressure. The pressure is doubled, (a) Will the equilibrium constant K change? (b) Will the number of moles of NO, O2 and N2, change? How?
Suppose the equilibrium constant of the reaction CO + 1/2O2 ↔ CO2 at 1500 K and 1 atm is K1. Express the equilibrium constant of the following reactions at 1500 K in terms of K1. (a) CO + (1/2)O2 ↔ CO2 at 2 atm, (b) CO2 ↔ CO + (1/2)O2 at 1 atm, (c) CO + O2 ↔ CO2 + (1/2)O2 at 1 atm, (d)
For the dissociation of nitrogen tetraoxide according to the reaction, N2O4 ↔ 2NO2, show that the degree of dissociation at equilibrium is given by ε = Ve/V0-1, where V0 is the initial volume and Ve is the equilibrium volume.
An equimolar mixture of carbon monoxide and water vapor at 1 atm and 298 K enters a reactor operating at steady state. The equilibrium mixture, composed of CO2, CO, H2O(g) and H2, leaves at 2000 K. Determine (a) Equilibrium composition of CO2 in the mixture, (b) The heat transfer (Q) between the
CO2 gas at 300 K and 400 kPa enters a steady state heat exchanger. An equilibrium mixture consists of CO2, O2, and CO exits at 2700 K and 350 kPa. Determine the (a) Composition of CO2 in the exiting mixture and (b) Heat transfer (Q) to the gas in kJ/kmol of CO2.
Carbon monoxide at 20oC and 100 kPa enters a combustion chamber and burns with 25% excess air entering at the same temperature and pressure. An equilibrium mixture consists of CO2, CO, O2, and N2 exits at 1200oC and 100 kPa. Determine The heat transfer (Q) to the surroundings in kJ/kmol of CO.
Methane (CH4) at 25oC and 1 atm enters a well-insulated reactor and reacts with air entering at the same conditions. For steady-state operation, negligible effects of ke and pe, and negligible pressure loss, plot the temperature of the combustion products against equivalent ratio ranging from 0.5
Repeat 14-4-12[BSW] if the reactants enter the chamber at 800oC and 1 atm.
Repeat 14-4-12[BSW] if the reactants enter the chamber at 600oC and 10 atm.
Octane (C8H18) at 25oC, 1 atm enters a combustion chamber and reacts with 111% theoretical air entering at the same conditions. If the products exiting at 1800 K contains CO, CO2, CN, H, H2, H2O, HCN, O, O2, O3, OH, N, N2, N2O, NO and NO2, determine (a) The molar fraction of NO in the products, in
Octane (C8H18) at 25oC and 100 kPa enters a combustion chamber and reacts with 100% theoretical air entering at the same conditions. Determine the equilibrium flame temperature assuming the products contains CO, CO2, CN, H, H2, H2O, HCN, O, O2, O3, OH, N, N2, N2O, NO and NO2. Use the equilibrium
In problem 13-2-10 [BVF], an equilibrium mixture consisting of CO2, CO, H2, H2O and O2 exits at 2500 K, 100 kPa. Determine (a) Molar composition of CO2 at equilibrium and (b) The amount of heat transfer per kg of fuel.
Carbon dioxide gas at 1 atm, 298 K enters a reactor operating at steady state. If an equilibrium mixture of CO2, CO and O2 exits at 2800 K, 1 atm, determine (a) The composition of the CO2 in the products and (b) The heat transfer to the surroundings per unit mass of carbon dioxide.
Hydrogen is heated in an open-steady device at 100 kPa from 300 K to 3000 K at a rate of 0.5 kg/min. Determine the rate of heat transfer in kW, assuming (a) No dissociation takes place, (b) Dissociation takes place.
An equimolar mixture of CO2, O2, and N2 enter a reactor operating at steady state. An equilibrium mixture of CO2, O2, N2, NO, and CO exits at 3500 K and 600 kPa. Determine the (a) Molar amount of CO2 (in kmols) in the mixture and (b) Heat transfer (q) to the surroundings per unit mass of CO2.
Hydrogen (H2) is heated during a steady-flow process at 1 atm from 298 K to 3000 K at a rate of 0.6 kg/min. Determine the rate of heat transfer needed during this process, assuming (a) Some H2 dissociates into H and (b) No dissociation takes place.
Carbon at 300 K, 100 kPa enters a chamber and reacts with oxygen entering at the same molar flow rate at 400 K, 100 kPa. An equilibrium mixture consists of CO2, CO, and O2 exits at 3000 K, 100 kPa. Determine the heat transfer to the surroundings in kJ/kmol of carbon.
Steam enters a heat exchanger operating at steady state. An equilibrium mixture of H2O, H2, O2, H, and OH exits at 2500 K and 100 kPa. Determine the (a) Equilibrium composition of H2O (in kmols) and (b) Heat transfer (q) to the surroundings per unit mass of steam. Assume the surroundings to be
Propane gas (C3H8) at 300 K and 100 kPa enters combustion chamber operating at steady state and reacts with 100% of excess air entering at 350 K and 100 kPa. An equilibrium mixture consists of CO2, CO, H2O(g), H2, O2, and N2 exits at 1100 K and 100 kPa. Determine The heat transfer (Q) to the
Methane gas (CH4) at 300 K and 100 kPa enters combustion chamber operating at steady state and reacts with 50% of excess air entering at 400 K and 100 kPa. An equilibrium mixture of CO2, CO, H2O(g), H2, and N2 exits at 2000 K and 100 kPa. Determine The heat transfer (Q) to the surroundings in
Two thermodynamics books, each with a mass of 1 kg, are stacked one on top of another. Neglecting the presence of atmosphere, draw the free body diagram of the book at the bottom to determine the vertical force on its (a) Top (b) Bottom faces in kN.
A vertical piston cylinder device contains a gas at an unknown pressure. If the outside pressure is 100 kPa, determine (a) The pressure of the gas if the piston has an area of 0.2 m2 and a mass of 20 kg. Assume g = 9.81 m/s2. (b) What-if Scenario: What would the pressure be if the orientation of
Determine the mass of the weight necessary to increase the pressure of the liquid trapped inside a piston-cylinder device to 120 kPa. Assume the piston to be weightless with an area of 0.1 m2, the outside pressure to be 100 kPa and g = 9.81 m/s2.
A mass of 100 kg is placed on the piston of a vertical piston-cylinder device containing nitrogen. The piston is weightless and has an area of 1 m2. The outside pressure is 100 kPa. Determine (a) The pressure inside the cylinder. The mass placed on the piston is now doubled to 200 kg. Also,
A piston with a diameter of 50 cm and a thickness of 5 cm is made of a composite material with a density (ρ) of 4000 kg/m3.(a) If the outside pressure is 101 kPa, determine the pressure inside the piston-cylinder assembly if the cylinder contains air.(b) What-if Scenario: What would the inside
A piston-cylinder device contains 0.02 m3 of hydrogen at 300 K. It has a diameter of 10 cm. The piston (assumed weightless) is pulled by a connecting rod perpendicular to the piston surface. If the outside conditions are 100 kPa and 300 K, (a) Determine the pull force necessary in kN to create a
Air in the accompanying piston-cylinder device is in equilibrium at 200oC. If the mass of the hanging weight is 10 kg, atmospheric pressure is 100 kPa, and the piston diameter is 10 cm, (a) Determine the pressure of air inside. Assume g = 9.81 m/s2 (b)What-if Scenario: What would the pressure be
A vertical hydraulic cylinder has a piston with a diameter of 100 mm. If the ambient pressure is 100 kPa, determine the mass of the piston if the pressure inside is 1000 kPa.
Determine the pull force necessary on the rope to reduce the pressure of the liquid trapped inside a piston cylinder device to 80 kPa. Assume the piston to be weightless with a diameter of 0.1 m, the outside pressure to be 100 kPa, and g = 9.81 m/s2.
A piston-cylinder device contains 0.17 m3 of hydrogen at 450oC. It has a diameter of 50 cm. The piston (assumed weightless) is pulled by a connecting rod perpendicular to the piston surface. If the outside conditions are 100 kPa, 25oC, (a) Determine the pull force necessary in kN to create a
A 5 cm diameter piston-cylinder device contains 0.04 kg of an ideal gas at equilibrium at 100 kPa, 300 K occupying a volume of 0.5 m3. Determine (a) the gas density (ρ), and (b) the specific volume (v). (c) A weight is now hung from the piston (see figure) so that the piston moves down to a new
Determine: (a) The pressure felt on your palm to hold a textbook of mass 1 kg in equilibrium. Assume the distribution of pressure over the palm to be uniform and the area of contact to be 25 cm2. (b) What-if Scenario: How would a change in atmospheric pressure affect your answer (0: No change; 1:
The lift-off mass of a Space Shuttle is 2 million kg. If the lift off thrust (the net force upward) is 10% greater than the minimum amount required for a lift-off, determine the acceleration.
A body weighs 0.05 kN on earth where g = 9.81 m/s2. Determine its weight on (a) The moon. (b) On mars with g = 1.67 m/s2 and g = 3.92 m/s2, respectively.
Calculate the weight of an object of mass 50 kg at the bottom and top of a mountain with (a) g = 9.8 m/s2 and (b) g = 9.78 m/s2 respectively.
According to Newton's law of gravity, the value of g at a given location is inversely proportional to the square of the distance of the location from the center of the earth. Determine the weight of a textbook of mass 1 kg at (a) sea level and (b) in an airplane cruising at an altitude of 45,000
The frictional force on a block of mass mA resting on a table (see accompanying figure) is given as F = μN, where N is the normal reaction force from the table. Determine the maximum value for mB that can be supported by friction. Assume the pulley to be frictionless.
If the block A in problem 0-1-7 [UJ] sits on a wedge with an angle θ with the horizontal, how would the answer change?
A block with a mass of 10 kg is at rest on a plane inclined at 25o to the horizontal. If μs = 0.6, determine the range of the horizontal push force F if the block is (a) About to slide down (b) About to slide up.
What do you call a system that has (a) No mass interaction. (b) No heat interaction. (c) No mass and energy interaction?
A hot block of solid is dropped in an insulated tank of water at the temperature of the surroundings. Determine the sign (positive: 1; negative: -1; none: 0) of Q treating (a) The block as the system. (b) The water as the system. (c) The entire tank (with the block and water).
An insulated tank containing high pressure nitrogen is connected to another insulated tank containing oxygen at low pressure. Determine the possible interactions as the valve is opened and the two gases are allowed to form a mixture by treating (a) One of the tanks as a system (b) Two tanks
A fluid is accelerated by an insulated nozzle attached at the end of a pipe. Identify the interactions, treating the nozzle as an open system.
An insulated steam turbine produces Q and Wsh as steam flows through it, entering at a high pressure and a high temperature and leaving at a relatively low pressure. Identify the interactions between the turbine (as an open system) and its surroundings and determine the sign (positive: 1; negative:
Identify the possible interactions of a steam turbine with poor insulation with its surroundings and determine the sign (positive: 1; negative: -1; none: 0) of(a) Q(b) Wext.
The pressure of a liquid flow is raised by a pump driven by an electrical motor. Identify the interactions treating(a) The pump as an open system.(b) The pump and the motor as a combined system.
An insulated compressor raises the pressure of a gas flow. The temperature of the gas is also increased as a result. Identify the possible interactions between the compressor and its surroundings and determine the sign (positive: 1; negative: -1; none: 0) of(a) Q(b) Wext.
In a heat exchanger (see accompanying animation) a flow of hot air is cooled by a flow of water. Identify the interactions treating(a) The entire heat exchanger as the system(b) One of the streams as the system.
A pressure cooker containing water is heated on a stove. Determine the interactions and signs (positive: 1; negative: -1; none: 0) of(a) Q (b) Wext, if any, as steam is released.
As shown in the figure below, electric current from the photovoltaic (PV) cells runs an electric motor. The shaft of the motor turns the paddle wheel inside the water tank. Identify the interactions (mass, heat, work) for the following systems:(a) PV cells.(b) Motor.(c) Tank.(d) The combined system
As you blow up a balloon, what are the interactions and the sign (positive: 1; negative: -1; none: 0) of(a) Q(b) Wext, if any, between the balloon as a system and its surroundings?

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