A cylinder contains 4 mol of an ideal gas at
30oC. If it expands from an initial...
A cylinder contains 4 mol of an ideal gas at
30oC. If it expands from an initial volume of
1.0 m3 to 2.0 m3 while maintained at a
constant pressure of 200 kPa.
What is the change in the temperature of the gas?
How much heat is absorbed or released from the system, over the
process?
The pressure is then reduced while the
gas is held at a constant volume.
If over this process the gas is returned to its original
temperature, what is the heat absorbed or released, over that
process?
An ideal monatomic gas expands adiabatically from an initial
temperature of 384 K and volume of 4.6 m3 to a final
volume of 10 m3. If the initial pressure is 1.5 ?
Patm, how much work is done on the gas?
A piston-cylinder apparatus contains initially 1.2 mol of ideal
gas at 6 bar and 25°C. Then the piston is moved downward to
increase the pressure to 12 bar pressure. You can ignore the change
in potential energy associated with the piston moving.
a. Write the First Law of Thermodynamics and simplify for this
problem given that temperature of the system changes.
b. Assuming Isothermal operation what are the initial and final
volumes of gas for the above process (L)?
c....
A 6.79-L cylinder contains 2.00 mol of gas A and 3.96 mol of gas
B, at a temperature of 31.5 °C. Calculate the partial pressure of
each gas in the cylinder. Assume ideal gas behavior.
A monatomic ideal gas has an initial temperature of 381 K. This
gas expands and does the same amount of work whether the expansion
is adiabatic or isothermal. When the expansion is adiabatic, the
final temperature of the gas is 290 K. What is the ratio of the
final to the initial volume when the expansion is isothermal?
A gas cylinder contains 2.30 mol He, 1.35 mol Ne, and 1.75 mol
Ar. If the total pressure in the cylinder is 2290 mmHg, what is the
partial pressure of each of the components? Assume constant
temperature.
P(He) = ?
P(Ne) = ?
P (Ar) = ?
4. 0.25 moles of an ideal gas expands from 72 mL to 10 L. For
each of the following experimental conditions, calculate U, q, and
w, each in Joules.
a. Gas expands in a vacuum under isothermal conditions.
b. Gas expands isothermally in Denver, Colorado, where the
constant external pressure is 675 Torr.
c. Gas expands isothermally in a reversible manner at 19 °C.
d. Gas expands adiabatically against a constant pressure of 760
Torr
A cylinder with a moveable piston contains 0.553 mol of gas and
has a volume of 256 mL .
What will its volume be if an additional 0.246 mol of gas is
added to the cylinder? (Assume constant temperature and
pressure.)
A cylinder contains 0.250 mol of carbon dioxide (CO2)gas at a
temperature of 27.0?C. The cylinder is provided with a frictionless
piston, which maintains a constant pressure of 1.00 atm on the gas.
The gas is heated until its temperature increases to 127.0?C.
Assume that the CO2 may be treated as an ideal gas.
a.) How much work W is done by the gas in this
process?
b.) What is the change in internal energy ?U
of the gas?
c.)...
An ideal gas expands isobarically (constant pressure) from point
A to point B. The gas is compressed isothermally (constant
temperature) from point B to C. Finally, the gas goes through an
isochoric (constant volume) process until it returns to point A.
Given: Volume at point A = Volume at point C = 0.004 m3,
Volume at point B = 0.008 m3, Pressure at point A =
Pressure at point B = 1,000,000 Pa, Temperature at point A = 600
K....
A piston and cylinder device (closed system) contain 2.25 mol of
an ideal gas which
is compressed irreversibly at constant temperature from 423 K and
200 kPa to 8 bar.
The irreversible work applied for the compression is 15 % larger
than the reversible
work for the same process. Determine the entropy change of the gas,
the
surroundings and the total entropy change if the heat is rejected
from the gas to
surroundings maintained at 25 oC.