Engineering Thermodynamics – CHE/CEEN/MEEN 2300 Test 4 Chapter 7 100 pts. You may use a calculator, the Properties Table booklet and a 3”x5” index card of formulas. Please show your work. Answers without supporting calculations will be counted wrong. 1. 20 pts A rigid tank contains an ideal gas at 300C that is being stirred by a paddle wheel. The paddle wheel does 100 kJ of work on the ideal gas. It is observed that the temperature of the ideal gas remains constant during this process as a result of heat transfer between the system and the surroundings at 200C. Use the table to organize your data State 1 State 2 T1 = 30 C T2 = 30 C V1 = V2 therefore v1 = v2 v2 = v1 a. 4 pts Determine the change in internal energy of the system Both the temperature and the specific volume are the same at State 1 and State 2, therefore the two states are identical, and all of the physical properties are the same at both states. Therefore, there is no change in internal energy. b. 4 pts Determine how much heat was transferred to the surroundings Perform an energy balance on the system (which is a closed system) Qin – Wout = ΔU = 0 therefore Qin must equal Wout and conversely, Qout must equal Win. Thus 100 kJ was transferred to the surroundings. c. 6 pts Determine the change in entropy of the system As shown in part a, the two states are identical. Therefore there is no change in entropy of the SYSTEM. This does not mean that the process does not result in a change in entropy – since the surroundings were affected by the process. You may wonder how there can be no change in entropy in the system, if there was heat transfer. The paddle wheel caused an increase in entropy, as it interacted with the gas in the system. Heat transfer caused a reduction in entropy. The two processes cancelled out!! d. 4 pts Determine the change in entropy of the surroundings The surroundings remained at constant temperature, therefore ΔS = Qsurroundings/T = 100 kJ/(20+273) K = 0.34 kJ/K Several students forgot that the temperature must be expressed in Kelvin. e. 2 pts Determine the change in entropy of the universe (Sgen) ΔSuniverse = Sgen = ΔSsystem + ΔSsurroundings = 0 + 0.34 kJ/K = 0.34 kJ/K 2. 20 pts A 0.5 m3 rigid tank contains R-134a initially at 200 kPa and 40% quality. Heat is transferred now to the refrigerant from a source at 350C until the pressure rises to 400 kPa. Use the table below to keep track of your properties State 1 P1 = 200 kPa x1 = 0.4 v1 = 0.0402 m3/kg u1 = 110.586 kJ/kg s1 = 0.459 kJ/kg K State 2 P2 = 400 kPa x2 = .786 v2 = 0.0402 m3/kg u2 = 195.56 kJ/kg s2 = 0.7701 kJ/kg K a. 4pts Find the mass of refrigerant in the system m = V/v v = vf + x vfg = 0.0007532 + 0.4 * (0.0993 – 0.0007532) = 0.0402 m3/kg m = 0.5 m3/0.0402 m3/kg = 12.44 kg b. 4 pts Find the total change in internal energy of the system ΔU = m Δu = m(u2 – u1) u1 = uf + x ufg = 36.69 + 0.4 * (221.43 – 36.69) = 110.586 kJ/kg Now we need to find u2, but we don’t know the value of x2. We can use the specific volume to help us v2 = vf +x2 vfg = 0.0007907 + x2 * (0.051201 – 0.0007907) = 0.0402 m3/kg x2 = 0.78 u2 = uf + x ufg = 61.69 + 0.786 * (231.9 – 61.69) = 195.56 kJ/kg ΔU = 12.44kg * (195.56 – 110.586) = 12.44 kg * (84.96 kJ/kg) = 1057 kJ c. 2 pts Find the amount of heat added to the system Perform an energy balance. Q – W = ΔU W=0 Q = ΔU = 1057 kJ d. 4 pts Find the change in entropy of the system ΔS = m Δs = m(s2 – s1) s1 = sf + x sfg = 0.1481 + 0.4 * (0.9253 – 0.1481) = 0.459 kJ/kg K s2 = sf + x sfg = 0.2399 + 0.786 * (0.9145 – 0.2399) = 0.7701 kJ/kgK ΔS = 12.44 kg * (0.7701 – 0.459) kJ/kg K = 12.44 kg * 0.3111 kJ/kg K = 3.87 kJ/K e. 4 pts Find the change in entropy of the heat source (which is large enough to stay at constant temperature) ΔS = Q/T = - 1057/(35 + 273) = -3.432 kJ/K f. 2 pts Find the change in entropy of the universe due to this process (Sgen) ΔSuniverse = Sgen = ΔSsystem + ΔSsurroundings = 3.87 – 3.432 = .44 kJ/K 3. 20 pts A 25 kg iron block initially at 3500C is quenched in an insulated tank that contains 100 kg of water at 180C. Assuming that the water that vaporizes during the process condenses back into the tank, determine the total entropy change during this process. Use the table to organize your data. water m = 100 kg iron m = 25 kg State 1 State 2 State 1 State 2 T1 = 18 C Tf = 26.66 C T1 = 350 C Tf = 26.66 C C = 4.2 kJ/kg K C = 0.45 kJ/kg C First, solve for the final temperature mH2O CH2O ΔTH2O = - miron Ciron ΔTiron 100 kg * 4.2 kJ/kg K * (Tf – 18) = - 25 kg * 0.45 kJ/kg K * (Tf – 350) Tf = 26.66 C For solids and liquids (incompressible materials) ΔS = m C ln(T2/T1) and ΔS system = ΔSH2O + ΔSiron ΔSH2O = 100 kg* 4.2 kJ/kg K[ (26.66 + 273)/(18 + 273)] = 12.31 kJ/K ΔSiron = 25 kg * 0.45 kJ/kg K ln[ 26.66 + 273)/(350 + 273)] = - 8.24 kJ/K ΔS system = 4.07 kJ/K 4. Air is compressed steadily by a 5 kW compressor from 100 kPa and 170C to 600 kPa and 1670C at a rate of 1.6 kg/min. During this process, some heat transfer takes place between the compressor and the surrounding medium at 170C. Use the table to keep track of your properties Inlet conditions Exit conditions Pi = 100 kPa Pe = 600 kPa Ti = 17 C + 273 = 290 K Te = 167 C + 273 = 440 K 0 si = 1.66802 kJ/kg K se0 = 2.08870 kJ/kg K hi = 290.16 kJ/kg he = 441.61 kJ/kg a. 8 pts Determine the rate of entropy change of air during this process Δs = cp avg ln(TeTi) - R ln(Pe/Pi) if you assume that the heat capacity is constant. A more accurate approach is: Δs = se0 – si0 - R ln(Pe/Pi) Δs = 2.08870 – 1.66802 - 0.2870 * ln(600/100) = -0.0935 kJ/kg K ΔS = m Δs = 1.6 kg/min * (-0.0935 kJ/kg K) = -0.1497 kJ/K min = -.0025 kJ/K sec b. 8 pts Determine the rate of entropy change of the surroundings due to heat transfer with the compressor First determine the rate of heat transfer into the system Q-W = m(Δh) (I’ve left off the dot to make it easier to type, but these are rates) Q = W + m(Δh) = - 5kJ/sec + 1.6 kg/min* min/60 sec*(441.61 – 290.16)kJ/kg = -.96 kJ/s Therefore the rate of heat transfer into the surroundings is + 0.96 kJ/sec ΔSsurroundings = Q/T = 0.96 kJ/s / (17 + 273) K = 0.0033 kJ/K sec c. 4 pts Find the rate of change of entropy of the universe (Sgen) due to this process. ΔSuniverse = Sgen = ΔSsystem + ΔSsurroundings = -0.0025 + 0.0033 = .0008 kJ/Ksec 5. 20 pts Liquid water enters a 25 kW pump at 100 kPa pressure at a rate of 5 kg/sec. Determine the highest pressure the liquid water can have at the exit of the pump. (Neglect the kinetic and potential energy change of water, and take the specific volume of water to be 0.001 m3/kg w = Wdot/mdot = 25 kJ/sec / 5 kg/sec = 5 kJ/kg w = v ΔP = 5 kJ/kg = .001 m3/kg (Pe – 100 kPa) Pe = 5100 kPa 6. 20 pts Helium gas is compressed from 14 psia and 700F to 120 psia at a rate of 5 ft3/s. Determine the power input to the compressor, assuming the compression process to be a) isentropic W mw k 1 kRT1 P2 k w 1 k 1 P1 The first thing we’ll need to do is find the mass flow rate, using the ideal gas law. The mass was worth 4 pts. PV mRT m PV RT 14 psia *5 ft 3 / sec 0.493lbm / s psia * ft 3 2.6809 * 70 460 R lbmR Now find the work per unit mass (4 pts) k 1 1.667 1 1.667 1.667 *0.4961 BTU / lbm * R * 70 460 R kRT1 P2 k 120 w * 1 1 14 k 1 P1 1.667 1 895.2 BTU / lbm Total work = 0.493 lbm/sec * 895.2 BTU/lbm = 44.1 Btu/sec b) polytropic with n = 1.2 (4 pts) Same as a, but substitute n for k, which gives w = 679.3 BTU/lbm Total work = 33.5 Btu/sec c) isothermal (4 pts) w = RT ln(P2/P1) = 0.4961 Btu/lbm R * (70 + 460)R * ln(120/14) = 564.9 Btu/ lbm Total work = 27.85 Btu/sec The trend of these numbers make sense, since the most efficient compressors are isothermal, the least are isentropic, and the more realistic polytropic case should fall between the two values. d) ideal two stage polytropic with n=1.2 (4 pts) Px P2 P1 120*14 41 psia is the intermediate pressure. Each of the two compressors carries half the load, which is: n 1 1.2 1 1.2 1.2*0.4961 BTU / lbm * R * 70 460 R nRT1 Px n 41 w * 1 1 14 n 1 P1 1.2 1 309.31BTU / lbm The total for the two compressors is twice this value, 618.6 Btu/ lbm, and the power required is: W mw 0.0493lbm / sec*618.6 Btu / lbm 30.49 Btu / sec this makes sense, since it is not as good as isothermal, but better than a single stage polytropic case.