Question

One mole of an ideal gas is held at a constant volume of 7.5 liter. Find the change in pressure (Pf-Pi), in atm if the temperature increases by 16.3 degrees Celsius.

Answer #1

One mole of an ideal gas initially at temperature T0 reversibly
expands from volume V0 to 2V0,
(a) at constant temperature (b) at constant pressure.
Calculate the work, the heat, and change in internal energy of
the gas in each process.

Consider an ideal gas of 0.2 mole of argon atoms with an initial
volume of 0.8 Liter and a temperature of 300K.
a) The gas is thermally isolated and allowed to expand
adiabatically to a final volume of 1 Liter. Find the final
temperature of the gas after its adiabatic expansion.
b) With the gas at the temperature Tf that you calculated in
(a), it is now brought into contact with a large thermal reservoir
at 300K and equilibriates to...

The pressure, volume, and temperature of a mole of an ideal gas
are related by the equation PV = 8.31T, where
P is measured in kilopascals, V in liters, and
T in kelvins. Use differentials to find the approximate
change in the pressure if the volume increases from 10 L to 10.6 L
and the temperature decreases from 365 K to 360 K. (Note whether
the change is positive or negative in your answer. Round your
answer to two decimal...

One mole of an ideal gas initially at a temperature of
Ti = 5.6°C undergoes an expansion at a constant
pressure of 1.00 atm to nine times its original volume.?
(a) Calculate the new temperature
Tf of the gas.
_____ K
(b) Calculate the work done on the gas during the
expansion.?
_____kJ

One mole of an ideal gas initially at a temperature of
Ti = 7.6°C undergoes an expansion at a constant
pressure of 1.00 atm to three times its original volume.
(a) Calculate the new temperature
Tf of the gas.
K
(b) Calculate the work done on the gas during the
expansion.
kJ

One
mole of an ideal gas at 25 degrees celsius and one atmosphere
pressure expands adiabatically to twice its original volume, then
compresses isothermally back to the original volume, then proceeds
isochorically back to the initial conditions. How much work is done
by the gas?
work done by the ideal gas.

One mole of an ideal gas does 3000 J of work on its surroundings
as it expands isothermally to a final pressure of 1.00 atm and
volume of 25.0 L. Determine:
a) the initial volume ?
b) the temperature of the gas?
(Note: 1 atm = 1.01 x 105Pa, universal gas constant R
= 8.31 J/mol K, 1 L = 10-3m3)

If 1.33 moles of an ideal gas has a pressure of 3.53 atm, and a
volume of 38.49 L, what is the temperature of the sample in degrees
Celsius?

If 5.95 moles of an ideal gas has a pressure of 4.22 atm, and a
volume of 88.83 L, what is the temperature of the sample in degrees
Celsius?

If 9.76 moles of an ideal gas has a pressure of 1.84 atm, and a
volume of 70.61 L, what is the temperature of the sample in degrees
Celsius?

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 3 minutes ago

asked 21 minutes ago

asked 34 minutes ago

asked 41 minutes ago

asked 44 minutes ago

asked 45 minutes ago

asked 50 minutes ago

asked 53 minutes ago

asked 57 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago