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
c. which of the following are state functions: q, w, ΔU
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1. a 10 mol sample of ideal gas whose heat capacities are Cv= 20.8 J/K Mole...
I. (30 pts.) One mole of an ideal gas with constant heat capacities and ? 5/3 is compressed adiabatically in a piston-cylinder device from T1-300 K, pi = 1 bar to p2 = 10 bar at a constant external pressure Pext"- P2 -10 bar. Calculate the final temperature, T2, and W, Q. AU, AH for this process. 2. (20 pts.) Repeat problem 1 for an adiabatic and reversible compression. 3. (20 pts.) A rigid, insulated tank is divided into two...
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...
6. (10 marks) A sample of 3.00 mol of ideal gas with Cv,m = 2.5R undergoes the change of states shown in the following P-T diagram (a + b → → a). Calculate the amount of expansion work (w) involved in each segment. P (atm) irreversible 1.50 reversible irreversible 1.001 - 400 600 T(K)
3. (7pts.) A closed system contains one mole of an ideal gas with constant heat capacities and 5/3 at Ti 400 K. The gas undergoes a constant-pressure process during which it receives = 62355/ ofheat. Calculate the final temperature of the gas, T2, the work produced, w, and the entropy change, ΔS, for the process.
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...
A 2.00 mol sample of an ideal gas with a molar specific heat of CV = 5 2 R always starts at pressure 1.50 ✕ 105 Pa and temperature 250 K. For each of the following processes, determine the final pressure (Pf, in kPa), the final volume (Vf, in L), the final temperature (Tf, in K), the change in internal energy of the gas (ΔEint, in J), the energy added to the gas by heat (Q, in J), and the...
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 a monatomic ideal gas expands from 4 to 10 L at constant pressure of 1 atm. Assuming that Cp = 20.8 J/mol-K, calculate ΔH for this process.
1.95 mol of an ideal gas with CV = 3R/2 undergoes the following transformations from an initial state T = 290 K, P = 1.000 bar. Find q, w, ∆U, ∆H and ∆S for each transformation. a) A reversible adiabatic compression until the final temperature reaches 390 K.
Question 2 One mole of an ideal gas, initially at 30 C and 1 bar is changed to 130 °C and 10 bar by using two different mechanically reversible processes: 2.1 The gas is first heated at constant pressure until its temperature is 130 °C and then compressed isothermally to 10 bar. 2.2 The gas is first compressed isothermally to 10 bar and then heated at constant pressure to 13°C Calculate Q, W, AU, and AH for each case. Take...