For an ideal gas Cp = 8.58 cal/mole-degree. What will be the final volume and temperature when 2 moles of the gas at 20OC and 15 atm are allowed to expand adiabatically and reversibly to 5 atm pressure? Find w, Q, ∆U and ∆H for the process.
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subject:
2. For an ideal gas Cp = 8.58 cal/mole-degree. What will be the final
volume and temperature when 2 moles of the gas at 20OC and 15
atm are allowed to expand adiabatically and reversibly to 5 atm
pressure? Find w, Q, ∆U and ∆H for the process.
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- 1.0 mole of an ideal gas is initially at T1=298 and has volume of v1=2.0L. it is then reversibly expanded to V2=3.0L. assume Cp=5/2 R and Cv=3/2R. 1-calculate delta (T, H,U) and heat and work for both isothermal and adiabatic processes 2- calculate the initial and final pressure for isothermal and adiabtic processes.1. A perfect gas undergoes compression at constant temperature, which reduces its volumeby 3.08 dm3. The final pressure and volume of the gas are 6.42 bar and 5.38 dm3, respectively. Calculate the original pressure of the gas in (a) bar, (b) atm. 2. Consider an isothermal column of an ideal gas at 25oC. What must be the molar mass ofthis gas be if the pressure is 0.80 of its ground level value at (a) 10km and (b) 1km ? Please show complete solutions. A 2.50 mole sample of a perfect gas for which Cv,m = 3R/2 (assume constant over T-range) undergoes the following two-step process: (1) from an initial state of the gas described by T = 13 ºC and P = 1.75 x 105 Pa, the gas undergoes an isothermal expansion against a constant pressure of 3.75 x 104 Pa until the volume has doubled. (2) subsequently, the gas is cooled at constant volume. The temperature falls to -24ºC. Calculate q, w, ∆U, and ∆H for each step and for the overall process.
- A gas mixture contains one-third methane by volume (recall what that means in terms of mole%) and the balance oxygen at 350°C and 3.0 bar. Calculate the specific enthalpy of this stream in kJ/kg (not per kmol) relative to the pure components at 25°C and 1 atm. State clearly all assumptions.For the equilibrium system: H2O(g) + CO(g) <--> H2(g) + CO2(g). Delta heat of rxn: -42 kJ/mol and Kc=0.62 at 1260 K.0.10 mol each of water, CO, and CO2 (all at 1260 K) are placed in a sealed 1.0-Liter thermally-insulated vessel, which is also at 1260 K. When the system comes to equilibrium, which is true?-The temp & mass of CO would increase.-The temp & mass of CO would decrease.-The temp would remain constant & the mass of CO would increase.-The temp would increase and the mass of CO would decrease.-The temp would decrease and the mass of CO would increase.6. As shown in Figure, a gas within a piston-cylinder assembly undergoes a thermodynamic cycle consisting of three processes in series: Process 1-2: Compression with U 2 =U 1 . Process 2-3: Constant-volume cooling to p 3 =140 kPa,; V 3 =0.028 m^ 2 . Process 3 - 1 : Constant-pressure expansion with W 31 =10.5 kJ. For the cycle, W eycle =28.3 kJ . There are no changes in kinetic or potential energy. Determine (a) the volume at state 1, in m ^ 3 . (b) the work and heat transfer for process 1-2, each in kJ. (e) Can this be a power cycle? A refrigeration cycle? Explain.
- Please I need help. Be as detailed as possible. Thank you! An ideal gas is placed in a cylinder with a movable heavy piston. The gas inside the cylinder has an initial pressure of 1.2 x 105 N/m2 , an initial temperature of 280 K, and an initial volume of 1 x 10-3 m3. A stove underneath the cylinder transfer energy to the gas through heating, causing the volume of the gas to increase to 2 x 10-3 m3. Assume that the gas expands isobarically (at constant pressure). 1) Draw a qualitative energy bar chart showing the changes of the energy within the system.An automobile wheel contains air with a pressure of 3x10^5 Pa at 25 ° C. The sipop cover was removed and the air was expanded adiabatically against an external pressure of 105 Pa. What is the final temperature of the gas in the wheel? (It should be taken into account that the gas behaves ideally and the Cp value for air is 7 / 2R)A constant-volume tank initially contains 1 kmol of carbon monoxide CO and 3 kmol of oxygen O2 (no nitrogen) at 25°C and 2 atm. Now the mixture is ignited and the CO burns completely to carbon dioxide CO2. If the final temperature in the tank is 500 K, determine the final pressure in the tank and the amount of heat transfer. Is it realistic to assume that there will be no CO in the tank when chemical equilibrium is reached?
- A piston/cylinder arrangement contains one mole of an ideal gas (the system) initially at 10.0 atm pressure and 300 K, as shown in the accompanying illustration. Neglecting the mass of the piston, neglecting friction, and assuming isothermal conditions throughout, the pin restraining the piston is removed. For the resulting process: (g = 9.807 m sR7) (a) What is qsyst if the mass of the weight is zero? (b) What is qsyst if the mass of the weight is 100 kg? (c) What is qsyst if the mass of the weight is 1017.4 kg?Oxygen at 150 K and 41.64 atm has a tabulated specific volume of 4.684 cm3/g and a specific internal energy of 1706 J/mol.(a) The figure 1706 J/mol is not the true internal energy of one g-mole of oxygen gas at 150 K and 41.64 atm. Why not? In a sentence, state the correct physical significance of that figure. (The term “reference state” should appear in your statement.)(b) Calculate the specific enthalpy of O2 (J/mol) at 150 K and 41.64 atm, and state the physical significance of this figure. What can you say about the reference state used to calculate it?Q1) A constant volume tank contain 1 mole ofC7H14and 12 mole of O2 gas at a temperature of 25 °C and 1 bar. The contents of the tank is ignited and C7H14 is burned completely and final products temperature is found to be 1700 K. Determine the heat transfer during this process. ( take daltaHo = -47800 kJ/kg).