Question

Four kilomoles of a monoatomic idel gas are at a temperature of 300 K. The gas expands reversibly and isothermally to twice its original volume.

1) Sketch the process in the P-V plane.

2) Compute the work done by the gas.

3) Compute the heat supplied to maintain constant temperature. Note U=U(T).

Answer #1

The sketch is given below

2)

Work done by the gas

Now putting the given values, we get

3)

And for isothermal process, we have

So, the heat suppled

Ten liters of a monoatomic ideal gas at 25o C and 10
atm pressure are expanded to a final pressure of 1 atm. The molar
heat capacity of the gas at constant volume, Cv, is 3/2R and is
independent of temperature. Calculate the work done, the heat
absorbed, and the change in U and H for the gas if the process is
carried out
(1) isothermally and reversibly, and
(2) adiabatically and reversibly.
Having determined the final state of the...

1.3 mole of an ideal gas at 300 K is expanded isothermally and
reversibly from a volume V to volume 4V. What is
the change in entropy of the gas, in
J/K?

One mole of air is compressed from pressure P1 and temperature
T1 at
constant volume till its pressure is doubled. Then it is
expanded
reversibly and isothermally to the original pressure, and finally
restored
to the original temperature by cooling at constant pressure. Sketch
the
path followed by the gas, on a P-V diagram and calculate the net
work
done by the gas.

n = 2.58 mol of Hydrogen gas is initially at T = 376 K
temperature and pi = 1.88×105 Pa pressure. The gas is then
reversibly and isothermally compressed until its pressure reaches
pf = 8.78×105 Pa. What is the volume of the gas at the end of the
compression process? What would be the temperature of the gas, if
the gas was allowed to adiabatically expand back to its original
pressure?

Use these steps to answer the questions below:
Step 1: A sample of monoatomic ideal gas, initially at pressure
P1 and volume V1, expands isothermally and
reversibly to a final pressure P2 and volume
V2
Step 2: The ideal gas is compressed isothermally back to its
initial conditions using constant pressure.
Give the equation needed to solve for the following
Wsys (Step 1)
=
qsys (Step 2)
=

n = 3.50 mol of Hydrogen gas is initially at T = 309.0 K
temperature and pi = 2.34×105 Pa pressure.
The gas is then reversibly and isothermally compressed until its
pressure reaches pf = 8.91×105 Pa.
1. What is the volume of the gas at the end of the compression
process? 1.01×10-2
m^3
2. How much work did the external force perform?
3. How much heat did the gas emit?
4. How much entropy did the gas emit?
5....

10.0 L of an ideal diatomic gas at 2.00 atm and 275 K are
contained in a cylinder with a piston. The gas first expands
isobarically to 20.0 L (step 1). It then cools at constant volume
back to 275 K (step 2), and finally contracts isothermally back to
10.0 L (step 3).
a) Show the series of processes on a pV diagram.
b) Calculate the temperature, pressure, and volume of the system
at the end of each step in...

n = 3.50 mol of Hydrogen gas is initially at T = 310 K
temperature and pi = 3.22×105 Pa pressure.
The gas is then reversibly and isothermally compressed until its
pressure reaches pf = 7.51×105 Pa. What is
the volume of the gas at the end of the compression process??

n = 4.42 mol of Hydrogen gas is initially at T = 304.0 K
temperature and pi = 3.23×105 Pa pressure.
The gas is then reversibly and isothermally compressed until its
pressure reaches pf = 8.93×105 Pa. What is
the volume of the gas at the end of the compression process?
Tries 0/12
How much work did the external force perform?
Tries 0/12
How much heat did the gas emit?
Tries 0/12
How much entropy did the gas emit?
Tries...

. A container has n = 3 moles of a monoatomic ideal gas at a
temperature of 330 K and an initial pressure of three times the
atmospheric pressure. The gas is taken through the following
thermodynamic cycle: 1.- The gas is expanded isobarically (constant
pressure) to Vf = 2.5∙Vi. 2.- The pressure of the gas is decreased
isochorically (constant volume) to half of the initial value. 3.-
The gas is compressed isobarically back to its initial volume. 4.-
The...

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