Compute the values (in Joules) of w, q, ΔU, ΔH, ΔS,ΔA and ΔG for 1.5 mol of an ideal gas that undergoes a reversible isothermal compression from V1= 2L to V2= 1L at 298 K.
Compute the values (in Joules) of w, q, ΔU, ΔH, ΔS,ΔA and ΔG for 1.5 mol...
for 2.25 moles of an ideal gas in a reversible isothermal process calculate q, w Δu, Δh, Δg, Δs, and Δa in joules (J) if the volume changes from 10L to 100L
Question 12: (1 point) What are the values of q, w, ΔU, ΔH, ΔS, ΔSsurr, and ΔSuniv for the following a constant pressure process for a system containing 0.572 moles of CH3OH ? CH3OH(l, 26.0 ºC, 1.00 atm) ⟶ CH3OH(g, 118.0 ºC, 1.00 atm) Assume that the volume of CH3OH(l) is much less than that of CH3OH(g) and that CH3OH(g) behaves as an ideal gas. Also, assume that the temperature of the surroundings is 118.0 ºC. Data: Molar heat capacity for CH3OH(l), Cp,m...
1) Compute the following values (in Joules) of w,q, AE, AH, AS, AA, and AG for 2.00 mole of an ideal gas that undergoes a reversible isothermal (300K) expansion from P = 5.00 atm to P = 0.500 atm.
A 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).
For the values give for ΔH and ΔS, calculate ΔG foreach for each of the following reactions at 298 K. If the reactionis not spontaneous under standard conditions at 298 K, at whattemperature (if any) would the reaction become spontaneous? a) 2PbS(s)+3O2(g) ---> 2PbO(s)+2SO2(g) ΔH= -844kj ; ΔS = -165 J/K b)2POCl3(g)--->2PCl3(g)+O2(g) ΔH= 572kJ ; ΔS= 179 J/K
(3). A sample of 1.00 mol ideal gas molecules with Cp, m = 7/2 R is initially at p = 1.00 bar and V = 22.44 L and then put thought the following cycle in reversible processes: (a) constant-pressure expansion to twice its initial volume, (b) constant-volume cooling to its initial temperature, (c) isothermal-compression back to 1.00 bar. Calculate q, w, ΔU, ΔH, ΔS for each process and for the whole cycle. (20 pts)
(3). A sample of 1.00 mol ideal gas molecules with Cp, m = 7/2 R is initially at p = 1.00 bar and V = 22.44 L and then put thought the following cycle in reversible processes: (a) constant-pressure expansion to twice its initial volume, (b) constant-volume cooling to its initial temperature, (c) isothermal-compression back to 1.00 bar. Calculate q, w, ΔU, ΔH, ΔS for each process and for the whole cycle.
An ideal gas (1.82 moles) undergoes the following reversible Carnot cycle. (1) An isothermal expansion at Thot=850K from 3.20L to 20.40L. (2) An adiabatic expansion until the temperature falls to 298K. The system then undergoes (3) an isothermal compression and a subsequent (4) adiabatic compression until the initial state is reached. a. Calculate work and ΔS for each step in the cycle and its overall efficiency. b. Determine ΔH and ΔU for steps (1) and (2). c. Explain why ΔUcycle=...
Calculate ΔA for the isothermal compression of 1.70 mol of an ideal gas at 325 K from an initial volume of 50.0 L to a final volume of 10.0 L. Does it matter whether the path is reversible or irreversible?
6.00 mol of an ideal gas with Cv.m = 1.5R undergo a two-step process. Calculate q, w, ΔU, and ΔH for each step and for the total process. Step A: Isothermal compression at 305K under a constant pressure of 10.0 bar from an initial pressure of 2.00 bar. Step B: After step A, the system is cooled at constant volume to 285K. Thank you