Question

You have 1.3 moles of a fictitious ideal gas whose molar
specific heat values are C_{v} = 13.43 J/(mol·K) and
C_{p} = 21.74 J/(mol·K). The gas is heated from T = 26.5 °C
to T = 120.7 °C at a constant volume of 0.0306 m^{3}

1. How much work is done by the gas?

2. How much thermal energy (heat) flows into the gas?

3. What is the change in the internal energy of the gas?

Answer #1

28 moles of an ideal gas with a molar specific heat at constant
volume of cv=3.2R is initially in state "A" at pressure 73390 Pa
and volume 1.0 m3.
The gas then expands isobarically to state "B" which has volume
2.6?3m3.
The gas then cools isochorically to state "C".
The gas finally returns from state "C" to "A" via an isothermal
process.
What is the adiabatic constant γ for this gas?
What is Q during the expansion from "A" to...

A cylinder contains 1.5 moles of ideal gas, initially at a
temperature of 113 ∘C. The cylinder is provided with a frictionless
piston, which maintains a constant pressure of 6.4×105Pa on the
gas. The gas is cooled until its temperature has decreased to 27∘C.
For the gas CV = 11.65 J/mol⋅K, and the ideal gas
constant R = 8.314 J/mol⋅K.
1.Find the work done by the gas during this process.
2.What is the change in the internal (thermal) energy of...

Three moles of a monatomic ideal gas are heated at a constant
volume of 2.90 m3. The amount of heat added is 5.10 103 J.
(a) What is the change in the temperature of the gas?
_____K
(b) Find the change in its internal energy.
_____J
(c) Determine the change in pressure.
_____Pa

1)
A quantity of n moles of oxygen gas
(CV = 5R/2 and Cp =
7R/2) is at absolute temperature T. You increase
the absolute temperature to 2T. Find the change in
internal energy of the gas, the heat flow into the gas, and the
work done by the gas if the process you used to increase the
temperature is isochoric.
Express your answers in terms of the variables n,
R, and T separated by commas.
2)
Find the change...

Calculate the change in entropy for 3 moles of an ideal gas with
Cp=(9/2)R and Cv=(7/2)R, undergoing the
following quasi-static process. The gas is initially at T=350K, and
is being compressed from 4 m3 to 1 m3 in a
perfectly insulated container.

A 2.0 mol sample of ideal gas with molar specific heat
Cv = (5/2)R is initially at 300 K and 100 kPa pressure. Determine
the final temperature and the work done on the gas when 1.6 kJ of
heat is added to the gas during each of these separate processes
(all starting at same initial temperature and pressure: (a)
isothermal (constant temperature) process, (b) isometric (constant
volume) process, and (c) isobaric (constant pressure) process.
Hint: You’ll need the 1st Law...

Rectangular PV Cycle
A piston contains 260 moles of an ideal monatomic gas that
initally has a pressure of 2.61 × 105 Pa and a volume of
4.9 m3. The piston is connected to a hot and cold
reservoir and the gas goes through the following quasi-static cycle
accepting energy from the hot reservoir and exhausting energy into
the cold reservoir.
1. The pressure of the gas is increased to 5.61 × 105
Pa while maintaining a constant volume.
2....

2.25 moles of an ideal gas with Cv,m = 5R/2 are transformed
irreversibly from an intital state T=680 K and P= 1.15 bar to a
final state T = 298 K and P = 4.75 bar a) Calculate change in
internal energy, change in enthalpy, and change in entropy for this
process b) Calculate change in internal energy, change in enthalpy,
and change in entropy if this process was reversible.

Assume that one mole of a monatomic (CV,m = 2.5R) ideal gas
undergoes a reversible isobaric expansion at 1 bar and the volume
increases from 0.5 L to 1 L. (a) Find the heat per mole, the work
per mole done, and the change in the molar internal energy, ΔUm,
the molar enthalpy, ΔHm, for this process. b) What are the entropy
changes ΔSm of the system and of the surroundings? Is this process
spontaneous? Justify your answer.

1. Under constant-volume conditions, 4200 J of heat is added to
1.4 moles of an ideal gas. As a result, the temperature of the gas
increases by 103 K. How much heat would be required to cause the
same temperature change under constant-pressure conditions? Do not
assume anything about whether the gas is monatomic, diatomic,
etc.
2. A system gains 3080 J of heat at a constant pressure of 1.36
× 105 Pa, and its internal energy increases by 4160...

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