Question

The air within a piston equipped with a cylinder absorbs 545 J of heat and expands from an initial volume of 0.107 L to a final volume of 0.853 L against an external pressure of 1.00 atm. What is the change in internal energy of the air within the piston?

Answer #1

as
a system increases in volume, it absorbs 58.0 J of energy in the
form of heat from the surroundings. the piston is working against a
pressure of 0.556 atm. the final volume of the system is 56.3 L.
what was the initial volume of the system if the internal energy of
the system decreased by 101.7 J?

As a system increases in volume, it absorbs 56.0 J of energy in
the form of heat from the surroundings. The piston is working
against a pressure of 0.593 atm. The final volume of the system is
55.9 L. What was the initial volume of the system if the internal
energy of the system decreased by 100.4 J?

One gram-mole of ideal gas is contained in a piston-cylinder
assembly. Cp=(7/2)R, Cv=(5/2)R. The gas expands from 3 to 1 atm.
Heat of 1000J is transferred to the gas during the process.
External pressure maintains at 1 atm throughout. Initial
temperature of the gas is 300K. Find work and internal energy
change.

1.) A balloon is inflated with air from an initial volume of
0.149 L to 2.151 L against an external pressure of 1.027 atm. If
the inflation occurred under adiabatic conditions, then what is the
change in internal energy in J of the air in the surroundings?
2.)A fuel mixture in a piston chamber expands from 246 mL to
1507 mL at constant temperature against a vacuum. How much work is
done (joules)?
PLEASE WORK OUT IM COMPLETELY LOST!

A 0.2 m3 piston/cylinder contains air at 400 K and
400 kPa and receives heat from a constant temperature heat source
at 1300 K. The piston expands at constant pressure to a
volume of 0.6 m3. Determine the change of availability
of the system.

A 19.0-L volume of an ideal gas in a cylinder with a piston is
at a pressure of 2.8 atm. Enough weight is suddenly removed from
the piston to lower the external pressure to 1.4 atm. The gas then
expands at constant temperature until its pressure is 1.4 atm.
Find the change in enthalpy, ?H, for this change in
state.
Express your answer using two significant figures.
Find the heat, q, associated with this change in
state.
Express your answer...

A certain amount of chlorine gas was placed inside a cylinder
with a movable piston at one end. The initial volume was 3.00 L and
the initial pressure of chlorine was 1.64 atm . The piston was
pushed down to change the volume to 1.00 L. Calculate the final
pressure of the gas if the temperature and number of moles of
chlorine remain constant.
Enter a numerical answer only, in terms of
atm.
Please show all work

A gas is compressed from an initial volume of 5.40 L to a final
volume of 1.22 L by an external pressure of 1.00 atm. During the
compression the gas releases 120 J of heat. What is the change in
internal energy of the gas?

Consider a mixture of air and gasoline vapor in a cylinder with
a piston. The original volume is 30. cm3. If the combustion of this
mixture releases 943 J of energy, to what volume will the gases
expand against a constant pressure of 632 torr if all the energy of
combustion is converted into work to push back the piston?

One mole of nitrogen gas confined within a cylinder by a
piston is heated from 0°C to
852°C at 1.00 atm.
(a) Calculate the work of expansion of the gas in
joules (1 J = 9.87 × 10−3 L·atm).
Assume all the energy is used to do work. (Enter your
answer in scientific notation.)
(b) What would be the temperature change if the gas were
heated with the same amount of energy in a container of fixed
volume? (Assume the...

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