Question

Calculate q and w for a process where 1.7 mol of an ideal gas at 300 K is isothermally and reversibly compressed from the pressure of 1.5 bar to 2.5 bar. Also enter the sign of the calculated q and w value and what it means. (heat delivered or absorbed and work done or required)

Answer #1

A sample of 64.0 g of methane, CH4 (molecular mass
16.0 g/mol, assume ideal gas behaviour)) at 300 K and with an
initial pressure V1 = 1.00 m3 is
compressed isothermally and reversibly to a final volume
of 2.00L. Calculate DU, DH, w, and q

In this problem, 1.10 mol of an ideal gas at 300 K undergoes a
free adiabatic expansion from V1 = 12.3 L to V2 = 22.2 L. It is
then compressed isothermally and reversibly back to its original
state.
(a) What is the entropy change of the universe for the complete
cycle?
J/K
(b) How much work is lost in this cycle?
J

An ideal gas with γ=1.4 occupies 5.0 L at 300 K and 120 kPa
pressure and is heated at constant volume until its pressure has
doubled. It's then compressed adiabatically until its volume is
one-fourth its original value, then cooled at constant volume to
300 K , and finally allowed to expand isothermally to its original
state.
Find the net work done on the gas. W= ___J

An ideal gas with ?=1.4 occupies 3.0L at 300 Kand
100kPa pressure and is compressed adiabatically until its volume is
2.0 L. It's then cooled at constant pressure until it reaches 300
K, then allowed to expand isothermally back to stateA.
Find the net work done on the gas and Vmin?

One mole of an ideal gas expands reversibly and isothermally
from 10. bar to 1.0 bar at 298.15K.
(i)Calculate the values of w, q, ∆U and ∆H?
(ii)Calculate w if the gas were to have expanded to the same
final state against a constant pressure of 1 bar.

A cylinder contains an ideal gas at the temperature of 300 K and
is closed by a movable piston. The gas, which is initially at a
pressure of 3 atm occupying a volume of 30 L, expands isothermally
to a volume of 80 L. The gas is then compressed isobarically,
returning to its initial volume of 30 L. Calculate the work done by
gas: a) in isothermal expansion; b) in isobaric compression, c) in
the whole process; and d) Calculate...

In this problem, 1.00 mol of an ideal diatomic gas is heated at
a constant wolume from 300 to 6000 K. (a) Find the increase in the
internal energy of the gas, the work done by the gas, and the heat
absorbed by the gas. (b) Find the same quantities if the gas is
heated from 300 to 600 K at constant pressure. Use the first law of
thermodynamics and your results form (a) to calculate the work done
by...

You are given an ideal monatomic gas of N = 1.00 × 1023 atoms at
temperature T = 300K, and volumeV = 20 L. Find:
(a) The pressure in the gas in Pa.
(b) The work done in Joules when the gas is compressed slowly
and isothermally to half its volume.
(c) The change in internal energy of the gas in Joules during
process (b).
(d) The heat (in J) absorbed or given up by the gas during
process (b)....

An ideal gas with γ = 1.4 occupies 6.0 L at 300 K and 100 kPa
pressure. It is compressed adiabatically until its volume is 2.0 L.
It's then cooled at constant pressure until it reaches 300 K, then
allowed to expand isothermally back to its initial state.
a.) Find the net work done on the gas.
b.) Find the minimum volume reached.

A 0.505-mol sample of an ideal diatomic gas at 408 kPa and 309 K
expands quasi-statically until the pressure decreases to 150 kPa.
Find the final temperature and volume of the gas, the work done by
the gas, and the heat absorbed by the gas if the expansion is the
following.
(a) isothermal
final temperature K
volume of the gas
L
work done by the gas
J
heat absorbed
J
(b) adiabatic
final temperature K
volume of the gas L...

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