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- A sample consisting of 2.00 mole of an ideal monoatomic gas is expanded isothermally at 22oC from 22.8 dm3 to 31.7 dm3 against a constant external pressure equal to the final pressure of the gas. Calculate w, q, /\U and /\H for this process.One mole of a perfect gas expanded isothermally and reversibly at 0 °C from 1 to 1/10 bar. Calculate (1) w, (2) q, (3) AH, (4) AG and (5) 4S for the gas.Fine the change in entropy for isothermal and siobaroc processes ?
- One mole of a monatomic ideal gas begins in a state withP 5 1.00 atm and T 5 300 K. It is expanded reversiblyand adiabatically until the volume has doubled; then it isexpanded irreversibly and isothermally into a vacuumuntil the volume has doubled again; and then it is heatedreversibly at constant volume to 400 K. Finally, it is compressed reversibly and isothermally until a inal state withP 5 1.00 atm and T 5 400 K is reached. Calculate DSsysfor this process. (Hint: There are two ways to solve thisproblem—an easy way and a hard way.)A sample of 1.00 mol perfect gas molecules with Cp,m = 7/2R is put through the following cycle: (a) Constant pressure heating to twice its initial volume, (b) Reversible, adiabatic expansion back to its initial temperature, (c) reversible isothermal compression back to its initial pressure. Calculate q, w, AU, and AH for each step and overall. Assuming the initial temperature and volume is P₁ and V₁.One mole of a perfect gas expanded isothermally and reversibly at 0 °C from 1 to 1/10 bar. Calculate (a) w, (b) q, (c) AH, (d) AG and (e) 4S for the gas.
- 2.0 atm adiabatic isothermal 16.0 L 40.0L V A thermodynamic cycle of 1.000 mol of monoatomic perfect gas (Cv,m = 12.47 JK1 mol1) consist of the following 3 stages: STAGE 1:1 to Il ; adiabatic reversible expansion from(T1 =273K, V:= 16.0 L, P1= 2.00 atm) to (T2= ?, P2=1atm, V2= 40.0 L) STAGE 2, Il to Il ;isothermal reversible compression from (T2 =?, V2 = 40L, P2 = 1.00 atm) to (T3 = ?, V3 = 16L, P3=?) STAGE 3: IIII to l; isochoric heating from (T3 =?, V3 = 16 L, P3 = ?) to (T1 = 273K, V = 16 L, P1 = 2 atm) What is the Stage 1 final temperature, T,? Answer in Kelvin in 3 significant figures. Type your answer. What is the change in internal energy (in kJ) in the Stage 1 process? Answer in 3 significant figures. Type your answer. 2 points Calculate q (in kJ) for the Stage 2 process. Answer in 3 significant figures. Type your answer. point Calculate q (in kJ) for the stage 3 process. Answer in 3 significat figures Type your answer. What is the overall change in internal energy (in kJ) for…2.25 moles of an ideal gas with Cv, m = 5R/2 are trans-formed from an initial state T= 680. K and P= 1.15 bar to afinal state I'= 298 K and P= 4.75 bar. Calculate for this pro-cess: AH & AS.I mol of per feet gas molecules at 27°c is expanded reversibly isothermally from an lnitial pressure o 3.00 atm to final pressure of 1.00 atm, determine the Value 9,W, DEDH, DS, OSur. DS .
- A mole of perfect monoatomic gas is expanded adiabatically and reversibly from 1 bar and 300K to 0.1 bar. Calculate the AS of the system in kJ7:53 PM Mon Nov 21 8) A sample of 1 mol of perfect gas at 298 K and 1 bar with Cvm = 3/2 R and Cp.m= 5/2 R is put through the following cycle: (a) constant-volume heating to twice its initial pressure, (b) reversible, adiabatic expansion back to its initial temperature, (c) reversible, isothermal compression back to 1 bar. Calculate q, w, AU, and AH for each step, as well as any necessary variables (e.g. V₁, T, etc.) n=1 mol T= 298 K P= I bar Cum 3R - 2 Cp.m-2R T b) a) w=0 n=1 T= 298 K Cvm = 3R 2 AP= 1 bar 9,² AU= ΔΗ: PV = nRT V = nRT @87% 8A sample of 1.00 mol perfect gas molecules with Cp,m = 7/2R and at 298 K and 1.00 atm is put through the following cycle: (a) Constant volume heating to twice its initial pressure, (b) Reversible, adiabatic expansion back to its initial temperature, (c) reversible isothermal compression back to 1.00 atm. Calculate q, w, ΔU, and ΔH for each step and overall (assume the initial temp is 298 K). Please answer very soon will give rating surely All questions answers needed Please answer complete questions