1. A gas (1.00 mol) obeying the following equation of state (EOS) is compressed from P...
1. A gas (1.00 mol) obeying the following equation of state (EOS) is compressed from P = 1.00 atm to P = 2.00 atm isothermally (300K) and reversibly: nRT P = v nb (a) (5 points) Calculate the entropy change, AS. (b) (10 points) Calculate the amount of heat () and work (w) involved. What does the total energy change (AU) tell you about the internal energy of this system?
Question 4 (40 points) Assume that a non-ideal gas can be described by the following EoS, where a and b are constant: (p + a)V -RT The gas is isothermally and reversibly expanded from (p, Vi) to (p2, V2) Determine the following thermodynamic properties for this process: W, Q, AU, ΔΗ, ΔΑ, AG, ASgas and ΔSsurroundings.
A 2.60-mol sample of helium gas initially at 300 K, and 0.400 atm is compressed isothermally to 1.00 atm. Note that the helium behaves as an ideal gas. (a) Find the final volume of the gas. (b) Find the work done on the gas. (c) Find the energy transferred by heat.
PChem 6. 2.00 mol of a perfect gas at 35°C is expanded reversibly and adiabatically to 10 °C. Assuming the molar volume heat capacity Cm = 28.2 K mol, calculate the heat exchange, work, internal energy change, entropy change, and enthalpy change of the system. (20 pts)
A 2.60-mol sample of helium gas initially at 300 K, and 0.400 atm is compressed isothermally to 1.00 atm. Note that the helium behaves as an ideal gas. (a) Find the final volume of the gas.? m3 (b) Find the work done on the gas. kJ (c) Find the energy transferred by heat. kJ
A 0.565 mol sample of So, (g) initially at 298 K and 1.00 atm is held at constant volume while enough heat is applied to raise the temperature of the gas by 14.7 K. Type of gas Molar heat capacity at constant va (Cym) atoms linear molecules nonlinear molecules R 3R Assuming ideal gas behavior, calculate the amount of heat (q) in joules required to affect this temperature change and the total change in internal energy, AU. Note that some...
Suppose 2.00 mol of an ideal gas of volume V =3.50m^3 at T = 300K .allowed to expand isothermally to V = 7.00m^3 at T = 300K. Determine (a) the work done by heat added to the gas. and (c) the change in internal energy of the gas. (Ans: 3.6 times 10^3, J, 0, 3.6 times 10^3J)
A gas is compressed from an initial volume of 5.75L to a final volume of 1.24 L by an external pressure of 1.00 ATM. During the compression the gas releases 125 J of heat. What is the change in internal energy of the gas?
A gas is compressed from an initial volume of 5.75L to a final volume of 1.24 L by an external pressure of 1.00 ATM. During the compression the gas releases 125 J of heat. What is the change in internal energy of the gas?
1)A gas is compressed at a constant pressure of 0.800 atm from 8.00 L to 1.00 L. In the process, 410 J of energy leaves the gas by heat. (a) What is the work done on the gas? J (b) What is the change in its internal energy? J 2) A gas increases in pressure from 2.00 atm to 6.00 atm at a constant volume of 1.00 m3 and then expands at constant pressure to a volume of 3.00 m3...