The formulae needed are:
(P = pressure, R = Gas constant, T = temperature, q = heat change, w = work done, E = internal energy, H = enthalpy, A = helmholtz free energy, G = gibbs free energy, S = entropy, n = number of moles:
(in equ III, q and w represent heat taken up and work done on the system)
So, putting the values in each of the equations:
Pi = 5.00 atm, Pf = 0.500 atm, T = 300 K, R = 8.314 J K-1 mol-1 , n = 2.00 moles
i) w = -2.303 (2)(8.314 J K-1 mol-1 )(300 K)log(10) = - 11,488.3 J
ii) delE = 0
iii) q = -(- 11,488.3 J) = 11,488.3 J
iv) del H = 0
v) delS = 11,488.3 J / 300K = 38.3 J K-1
vi)del A = -(300 K)(38.3 J K-1) = - 11,488.3 J
vii) del G = - 11,488.3 J
You'll find that q, delA , delG and also w(if you consider magnitude) have same values.
These are because:
1) Compute the following values (in Joules) of w,q, AE, AH, AS, AA, and AG for...
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.
For a certain perfect gas, CV,m = 2.5R at all temperatures. Calculate q, w, ?U, ?H, and ?S when 2.00 mol of this gas undergoes each of the following processes: (a) a reversible isobaric expansion (1.00 atm, 20.0 L) to (1.00 atm, 40.0 L). (b) A reversible isothermal compression from (0.500 atm, 40.0 L) to (1.00 atm, 20.0 L).
1 mole 2. Compute w,q, and AU for the following processes by an ideal gas: 1) irreversible expansion against a constant external pressure of 2.00 atm from 5.00 L to 10.00 L at 30°C. 2) one irreversible compression using minimum external pressure to achieve the reverse process.
Consider the expansion of 1.00 mole of (ideal) Ne from 2.00 atm at 75.00 C: the volume is doubled in the process. Find q, w, Delta H and the final pressure and temperature for a) reversible adiabatic expansion b) reversible isothermal expansion c) reversible constant pressure expansion d) irreversible adiabat against 0.500 atm external pressure
1. a 10 mol sample of ideal gas whose heat capacities are Cv= 20.8 J/K Mole and Cv = 29.1 J/K Mole a. Undergoes a reversible constant volume cooking from 49.3 L, 300 K, and 5.00 atm to 150 K. Calculate q, w, and ΔU. b. the same gas then underwent a reversible constant pressure expansion from 150 K and 2.50 atm to 98.6 L. Calculate q , w, and ΔU. You'll need the ideal gas law to calculate T-final...
2. Compute w,q, and AU for the following processes by an ideal gas: 1) irreversible expansion against a constant external pressure of 2.00 atm from 5.00 L to 10.00 L at 30°C. 2) one irreversible compression using minimum external pressure to achieve the reverse process.
Obtain heat q and work w given to an ideal gas (1 moD system and the ehange of the internal energy Au in the following processes. Heat capacity at constant volume, G, of the gas does not 1. AU in t A reversible isothermal expansion from (P. V.,T) to (P, V, r). reversibly at constant volume from (Pvv2,T) to (p,y, ) depend on temperature. a) b) A reversible adiabatic expansion from (P, V.T) to (P, V, T2) and then heating...
Ten. moles of ideal gas (monatomic), in the initial state P1=10atm, T1=300K are taken round the following cycle: a. A reversible isothermal expansion to V=246 liters, and b. A reversible adiabatic process to P=10 atm c. A reversible isobaric compression to V=24.6 liters Calculate the change of work (w), heat (q), internal energy (U), and entropy (S) of the system for each process?
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
EXAMPLE 3.15. Calculate AU, q, w, and AH for the reversible compression of 2.00 mol of an ideal gas from 1.00 bar to 100.0 bar at 25°C.