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 ΔH for the overall process (at the end of the two stages).
One mole of an Ideal Gas, for which Cv,m = 3/2R, initially at 20.0 C and...
1.5 moles of an ideal gas, for which the molar heat capacity Cv.m = 3/2R, initially at 25.0°C and 1 atm undergoes a two-stage transformation. Calculate q. w. Au in kJ for the complete process (a+b). a. The gas is expanded isothermally and reversibly until the volume doubles b. Beginning at the end of the first stage, the temperature is raised to 100.0°C at constant volume. 9 -2.57 ki A. W = 2.57 kJ AU = 5.14 k) = +2.57...
Suppose that we allow 3.50 mol of an ideal gas with Cv=5R/2 to expand isothermally and reversibly from 100 atm, 10 L to 10.0 atm and then the gas is allowed to expand adiabatically and reversibly to a final pressure of 1.00 atm. Calculate q, w, ΔU and ΔH for each step and the total values for the two steps. Suppose now that the processes are carried out irreversibly with pressure dropping discontinuously from 100 atm to 10.0 atm in...
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...
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.
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 mole of ideal diatmic gas with Cv,m= 2.5 R at 27 C and .100 MPA is compressed adiabatically and reversibly to a final pressure of 1.00 MPa. Calculate the final temp, q,w, Delta U, and Delta H, and Delta S for the process.
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...
2. One mole of an ideal gas at an initial state of 300 K, 2.4618 atm and 10.0 L is isothermally expanded to 20.0 L against a constant external pressure of 1.2309 atm. Calculate AU, W, q, and AS for the process. Show that the Clausius inequality is satisfied.
2. One mole of an ideal gas at an initial state of 300 K, 2.4618 atm and 10.0 L is isothermally expanded to 20.0 L against a constant external pressure of 1.2309 atm. Calculate AU, W, q, and AS for the process. Show that the Clausius inequality is satisfied.
Q3d d) One mole of an ideal gas with Cu.m 3/2R is heated reversibly along a path such that V = Aexp[bT], where A = 1.2257 liters and b-0010 K-1. How does the pressure vary with T for this system? Obtain the molar heat capacity of the gas as a function of T for heating along the given path. Finally, if 2 moles of the gas are heated reversibly along this path from 300 to 400 K; compute AU, w,...