One mole of O2(g), with CV,m=2.5R, is expanded
adiabatically from 301 K and 4.00 bar to 1.60 bar against a
constant external pressure equal to the final pressure. Calculate
q, w, ΔU, ΔH, ΔS and ΔSsurr.
Enter your answers in the specified units with three or more
significant figures . Do not include units as part of your
answer.
q = ____________ J
w = ____________ J
ΔU = ____________ J
ΔH = ____________ J
ΔS = ____________ J mol-1 K-1
ΔSsurroundings = ____________ J mol-1 K-1
One mole of O2(g), with CV,m=2.5R, is expanded adiabatically from 301 K and 4.00 bar to 1.60...
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...
One mole of an Ideal Gas, for which Cv,m = 3/2R, initially at 20.0 C and 1.00 x106 Pa undergoes a two-stage transformation: Stage 1: The gas is expanded isothermally and reversibly until the volume doubles. Stage 2: Beginning at the end of the first stage, the temperature is raised to 80.0 C at constant volume. For each stage, calculate the final pressure, heat(q), work(w), change in internal energy (ΔU), and enthalpy (ΔH). Calculate the total q, w, ΔU, and...
One mole of an ideal gas with CP = (7/2)R and CV = (5/2)R expands from P1 = 8 bar and T1 = 630 K to P2 = 1 bar. Take the value of R as 8.314 J·mol-1·k-1. At constant volume (assume mechanical reversibility), find the value of W, Q, ΔU, and ΔH? rt.)
One-half mole of helium is expanded adiabatically and quasi-statically from an initial pressure of 4.00 atm and temperature of 540 K to a final pressure of 1.00 atm. Find the following values for the gas. a) the work done by the gas KJ b) the change in the internal energy KJ
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...
One mole of a gas is expanded from 0.1 bar to 0.01 bar at a constant temperature of 350 K. The gas obeys the equation of state p(Vm - b) = RT where b is a constant equal to 0.01 dm3 mol-1. Find ΔH in mJ for this process.
Consider a system consisting of 3.0 mol CO2(g), initially at 35°C and 9.0 atm and confined to a cylinder of cross-section 100.0 cm2. The sample is allowed to expand irreversibly and adiabatically against an external pressure of 2.5 atm until the piston has moved outwards through 25 cm. Assume that carbon dioxide may be considered a perfect gas with CV,m = 28.8 J K–1 mol–1, and calculate (a) q, (b) w, (c) ΔU, (d) ΔT, (e) ΔS.
Five moles of nitrogen gas is expanded in a piston-cylinder assembly from an initial state of 3 bar and 88 ºC to a final pressure of 1 bar. You can assume nitrogen to behave as an ideal gas with a constant heat capacity CP =7R/2. a) If the expansion is carried out isothermally and reversibly, calculate Q, W, ΔH and ΔU. Draw the process on a pV diagram. Label the axis and the path clearly. b) If the expansion is...
For a Van der Waals gas, the following equations hold. P = nRT/(V−nb) − a(n/V)2 dU = CV dT + a(n/V)2 dV For chlorine gas, CV,m = 25.6 J K−1 mol−1, a = 6.343 bar L2 mol−2, and b = 0.0542 L mol−1. Calculate q, w, ΔU, and ΔH, in joules, when one mole of chlorine gas is expanded isothermally and reversibly at 449 K from 7.0 L to 15.0 L.
A sample of 1.00 mol of N2 gas is expanded adiabatically from a volume of 10.00 dm3 and a temperature of 400 K to a volume of 20.00 - 3 -dm3. Assume that nitrogen is ideal, with Cv,m = 5R/2. (i) Find the final temperature if the expansion is carried out reversibly. (ii) Calculate the final temperature if the expansion is carried out with a constant external pressure of 1.00 atm. (iii) Find the final temperature if the gas expands...