One mole of an ideal monatomic gas is expanded from an initial state at 3 bar and 450 K to a final state at 2 bar and 250 K.
Choose two different paths for this expansion, specify them carefully, and calculate w and q for each path.
Calculate ?U and ?S for each path.
One mole of an ideal monatomic gas is expanded from an initial state at 3 bar...
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...
One mole of an ideal gas from an initial state described by T= 250 Kand P= 1.00 bar with CV,m= (5/2)Rundergoes an adiabatic expansion against a constant external pressure of 0.500 bar until the final pressure is half its initial value. What is w, and ΔS for this process? Note that the process involves both changes in T and P.
Calculations: (27 points) One mole of an monatomic ideal gas is initially at 12 bar and 298 K. It is allowed to expand against a constant external pressure of 4 bar to a final pressure of 4 bar. During this process, the temperature of the gas falls to 262 K. a. Find Δυ (6 points), ΔΗ (6 points), as (6 points).( Show your calculation) b. Draw three deferent paths in three P-V graphs, respectively, to accomplish the above thermodynamic change...
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.
In both cases below, one mole of an ideal gas is expanded from an initial volume V to a final volume 2 V. In both cases, the gas is identical and the initial pressure is 2P. The expansion is adiabatic in A and isothermal in B. Will the final temperature of the gas be (i) greater in Case A, (ii) greater in Case B, or (iii) the same in both cases? Explain your reasoning
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?
4. One mole of monoatomic ideal gas, initially at 27 oC and 1 bar, is heated and allowed to expand reversibly against constant pressure of 1 bar until the final temperature is 127 °C. 4.1 What are the initial (Vi) and final (V2) volumes of the gas? 4.2 Calculate the work (w) that the gas does during this expansion. 4.3 Calculate the internal energy change (AU) of this expansion process 4.4 Calculate the enthalpy change (AH) of this expansion process.
Consider the diagram below. The following is for an ideal monatomic gas Cvm 3/2 R State A: STP State B: P,T, V-midway between Vc and Va State C: P 1 atm, V-4VA, T Path 1: A circular path from state A to state B Path 2: Straight line paths from states A to B and B to C Calculate w, q, Δυ and ΔΗ for each of the following cases: (Give your answers in SI units) 1. Along Path 1...
For a reversible, adiabatic expansion of 1.00 mol of a monatomic ideal gas the initial and final conditions are shown in the following table and AE = W = -2.24 kJ. Initial 10.00 bar 2.478 L 298 K Final 1.00 bar 9.87 L 119 K Part A Find AH for this process. Express your answer to three significant figures and include the appropriate units. AH = Value Units Submit Request Answer