An ideal gas (R = 0.26 kJ/kg-K) initially at a pressure of 60 kPa and wolume of 0.1 m^3 is compressed isothermally at 25 degree Celsius to a pressure of 120 kPa. Calculate
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- A closed cylinder contains 1.0 mole of ideal monatomic gas at 300 oC and 4.0 bar.Insulating the cylinder so that there is no heat exchange with the surroundings, the gas isexpanded to 200 oC and 1.0 bar producing 1247 J of work.a) Is this process reversible or irreversible?b) What is the change in enthalpy (∆H) of the gas?c) What is the change in internal energy (∆U) of thegas?450 g of gaseous benzene (MW = 78.11 g/mol) is heated from 40 ⁰C to 1,050 ⁰C at constant pressure. Determine the change in entropy (in kJ/K). Specific heat capacity is not constant throughout the process.1 mol super cooled liquid water transformed to solid ice at -10 oC under 1 atm pressure. a) Calculate entropy change of the system, surrounding and universe. (temperature of the environment is -10 °C) b) Make some comments on entropy changes from the obtained data Please use the following data for water : Melting entalpy of ice (ΔHmelting) at 0°C and 1 bar is 6020 J mol-1. Cp (H2O (s)) = 37,7 J mol-1 K-1 Cp (H2O (l)) = 75,3 J mol-1 K-1
- 4. A sample consisting of 150 g of CO molecules at 300 K is expanded isothermally from an initial pressure of 5.0 bar to a final pressure of 2.0 bar. Calculate q, w, ∆U, ∆H, ∆Ssys, ∆Ssurr, and ∆Stotal for the process two ways: (a) reversibly and (b) irreversibly against a constant pressure of 2.0 bar. Cp,m is constant at a value of 29.14 J/mol* K, and temperature of the surroundings is 273 K. State whether each process is spontaneous.120 liters of acetylene (ρ = 1.05 kg/m³ @ 25 ⁰C) is heated from 25 ⁰C to 350 ⁰C at constant pressure. Determine the change in entropy (in J/K). Assume constant specific heat capacity throughout the process./A piston–cylinder device initially contains volume 0.015 m3 of ethane gas at 102 kPa & 22°C. The gas reversibly and adiabatically is compressed to 6.8 bar. Determine the work done during the process and the final temperature, the final volume, take CP = 1.005 kJ/kg .K, CV = 0.718kJ/kg .K?
- Consider one mole of a simple ideal gas enclosed in a cylindrical piston with rigid impermeable adiabatic walls. The piston has a cross sectional area ofA = 0.10 m^2 and the cylinder enclosing the gas has a height of h = 1.0 cm. The gas inside the piston has a temperature T = 300.K. Recall that the internal energy for an ideal gas is U= n cV,mT, where cV,m= 1.5 R is the molar heat capacity for the ideal gas. mass m = 15.3E3kg is placed on the top of the piston, but that the piston top remains rigid. The external pressure applied is 1.5E6 Pa. Determine the equilubrium volume for the gas.Consider one mole of a simple ideal gas enclosed in a cylindrical piston with rigid impermeable adiabatic walls. The piston has a cross sectional area ofA = 0.10 m^2 and the cylinder enclosing the gas has a height of h = 1.0 cm. The gas inside the piston has a temperature T = 300.K. Recall that the internal energy for an ideal gas is U= n cV,mT, where cV,m= 1.5 R is the molar heat capacity for the ideal gas. mass m = 15.3E3kg is placed on the top of the piston, but that the piston top remains rigid. The external pressure applied is 1.5E6 Pa. The equilubrium volume for the gas is 1.6E-3 m^3. Suppose that the piston is now allowed to move within the cylinder, but that the walls remain adiabatic and impermeable so that no heat flows into the gas. The gas system will ultimately move to a new equilibrium state. We will now characterize the final equilibrium state and the changes resulting from the process. Define the (Total System) = (the gas enclosed in the cylinder) plus (the mass placed…Pure water under the atmospheric pressure of 100,000 Pa is converted to steam at a temperature of 100 0C. What statement can you make regarding the relation between Gibbs free energy (or chemical potential) of water and steam at 100 0C, under atmospheric pressure. If the heat needed to vaporise 1 kg of water to steam at 100 0C is 2265 kJ/kg. Work out the difference between entropy of steam and water at the boiling temperature. b) If a small amount of salt 0.0002 mol is added to every 18 g of water, calculate the chemical potential change of water in the salt solution. c) Assuming that the chemical potential of water in the solution does not change much with pressure, work out the pressure at which the water in the salt solution will boil, at 100 0 You may take steam as being an ideal gas.
- 1. 0.1m3 of an ideal gas at 300 K and 1 bar is compressed adiabatically to 8 bar. It is then cooled at constant volume and further expanded isothermally so as to reach the condition from where it started. Determine the following with aid of a NEAT DIAGRAM a. Pressure at the end of constant volume cooling b. Change in internal energy during the constant volume process c. Net work done and heat transferred during the cycle. Assume, Cp = 14.3 kJ/kgK and Cv = 10.2 kJ/kgK.1.65 mol of a perfect gas for which Cv,m = 12.47 J K–1 mol–1 is subjected to two successive changes in state: (1) from 37.0 oC and 1.00´105 Pa, the gas is expended isothermally against a constant pressure of 16.5´103 Pa to twice its initial volume. (2) At the end of the previous process, the gas is cooled at constant volume from 37.0 oC to - 23.0 oC. (a) Calculate q , w , DU, DH for each of the stages.P3B.7 A block of copper of mass 500 g and initially at 293K is in thermalcontact with an electric heater of resistance 1.00 kΩ and negligible mass. Acurrent of 1.00A is passed for 15.0 s. Calculate the change in entropy of thecopper, taking Cp,m = 24.4 JK−1mol−1. The experiment is then repeated with thecopper immersed in a stream of water that maintains the temperature of thecopper block at 293K. Calculate the change in entropy of the copper and thewater in this case.P3B.8 A block of copper (Cp,m = 24.44 JK−1mol−1) of mass 2.00 kg and at0 °C is introduced into an insulated container in which there is 1.00molH2O(g) at 100 °C and 1.00 atm. Assuming that all the vapour is condensed toliquid water, determine: (a) the final temperature of the system; (b) the heattransferred to the copper block; and (c) the entropy change of the water, thecopper block, and the total system. The data needed are given in ExerciseE3B.7a.