(b) Consider an adiabatic, reversible expansion of 0 020 mol Ar (perfect gas), initially at 25...
Consider a reversible adiabatic expansion of 1.00 mol of an ideal gas, starting from 1.90 L and 415 K , if 2.0 kJ of work is done by the expansion. The molar heat capacity at constant volume of the gas is 2.5R. R = 8.314 JK−1mol−1. Determine the final temperature of the gas in the process. Determine the final volume of the gas in the process. Determine the final pressure of the gas in the process.
1 00 mol of a perfect gas initially at 1 00 atm and 298 K with Cpm (7/2) R is put through the following cycle () constant-volume heating to twice its initial temperature (u) reversible, adiabatic expansion back to its onginal temperature () reversible, isothermal compression back to 1 00 atm Calculate q, w, AU, and AH for each of the steps ()-(m) above Hints First calculate AU, then q AH easily follows Remember the meaning of an adiabatic process...
One mole of an ideal gas undergoes a reversible adiabatic expansion from T_1, to T_2 while tripling the volume of the gas. What is the relation between T_1 and T-2? T-2/3 < T_1<T_2 T_2/3 < T_1 < T-2 T_1= T_2 T_2<T_1 T_1 lessthanorequalto T_2/3 One mole of Ar gas undergoes the reversible transformation shown. Assuming Ar behaves ideally, which statement is true for step 2? Delta U= C_p DeltaT DeltaH < Delta U Delat S= c_p ln(T_c/T_B) W = etaRt...
2 140 pt) Reversible Adiabatic Expansion of Nitrogen. Nitrogen expands reversibly in an insulated cylinder fitted with a piston. The N2 is initially at 500K and 5 bar pressure and expands to a final pressure of 1 bar. Determine the final temperature T of the N2 (in K) as well as the work done in the process W (mol), assuming N2 to be in the ideal gas state. Heat capacity, Cp is equal to a constant at 3.560R.
By a reversible adiabatic expansion, temperature of an ideal gas (n mol) changed from T, to Ts Express the changes of the internal energy and enthalpy by using heat capacity at conatant volume, Cy 2.
During an adiabatic expansion the temperature of 0.490 mol of argon (Ar) drops from 64.0 °C to 10.0 °C. The argon may be treated as an ideal gas. How much work does the gas do? Express your answer with the appropriate units. t μΑ ? 288 W J Submit Previous Answers Request Answer X Incorrect; Try Again; 2 attempts remaining You may have forgotten that the process is adiabatic, not isobaric. Recall the definition of this process, and use the...
(b) The constant-pressure heat capacity of a sample of 1 00 mol of a perfect gas was found to vary with temperature according to the expression Cp/(J K)20 17 + 0 4001 (TK) Calculate q, w, AU and AH when the temperature is raised from 0°C to 100°C ) at constant pressure (u) at constant volume (10) (b) The constant-pressure heat capacity of a sample of 1 00 mol of a perfect gas was found to vary with temperature according...
During an adiabatic expansion the temperature of 0.480 mol of argon (Ar) drops from 55.0 degree C to 11.0 degree C. The argon may be treated as an ideal gas. How much work does the gas do? W = _______ What is the change in internal energy of the gas? Delta U = _____
For a reversible, adiabatic expansion of 1.00 mol of a monatomic ideal gas the initial and final conditions are shown in the following table and AE = W = -2.24 kJ. Initial 10.00 bar 2.478 L 298 K Final 1.00 bar 9.87 L 119 K Part A Find AH for this process. Express your answer to three significant figures and include the appropriate units. AH = Value Units Submit Request Answer
A sample of 1.00 mol perfect gas molecules with Cp,m = 7/2 R is put through the following cycle:(a) Constant-volume heating to twice its initial volume,(b) Reversible, adiabatic expansion back to its initial temperature,(c) Reversible isothermal compression back to 1.00 atm. Calculate q, w, ?U, and ?H for each step and overall.