Question

5 moles of a monatomic ideal gas initially at 1 atm and 200 K is compressed isothermally against a constant external pressure of 2.0 atm, to a final pressure of 2.0 atm. Calculate W; Q; U; and H in Joules.

Answer #1

Two moles of helium gas initially at 195 K and 0.32 atm are
compressed isothermally to 1.83 atm.
a) Find the final volume of the gas. Assume that helium behaves
as an ideal gas. The universal gas constant is 8.31451 J/K

4. Three moles of a monatomic ideal gas are initially at a
pressure of 1.00 atm and a temperature of 20.0OC. The gas is
compressed adiabatically to a final pressure of 5.00 atm. Find: (a)
the initial volume of the gas; (b) the final volume of the gas; (c)
the final temperature of the gas; (d) the work done by the gas
during the compression.
Answers: (a) 72.1 L; (b) 27.5 L; (c) 285 OC; (d) -97.8
atm-L
Please show...

5 mole of an ideal gas for which Cv,m=3/2R, initially at 20 oC
and 1 atm undergoes a two-stage transformation.
For each of the stages described in the following list,
Calculate the final pressure as well as q, w, ∆U, ∆H and ∆S.
a) The gas is expanded isothermally and reversibly until the
volume triple.
b) then, the temperature is raised to T=2000 oC at the constant
volume. Note: R= 8.314 j/mol.K or 0.082 lt.atm/mol.K, 1lt.atm=
101.325 joule

6. An ideal
monatomic gas initially at 26.85 K and 3.250 bar is added to a
1.750 L vessel. Assuming that the system consists of the ideal gas
alone, calculate the values of Vf, Tf, Pf, w, q, ΔU, and ΔH for
each of the following processes. Construct a table for each part
listing the initial and final value of V, T, and P and the value of
w, q, ΔU, and ΔH.

1 mole of ideal gas at 270C is expanded isothermally from an
initial pressure of 3 atm to afinal pressure of 1 atm in two ways:
(a) reversibly and (b) against a constant external pressure of 1
atm. Calculate q, w, ΔU, ΔH and ΔS for each path.

One mole of an ideal gas is compressed at a constant temperature
of 55 oC from 16.5 L to 12.8 L using a constant external
pressure of 1.6 atm. Calculate w, q, ΔH and ΔS for this
process.
w = (?) kJ
q = (?) kJ
ΔH = (?) kJ
ΔS = (?) J/(mol*K)

In this problem, 0.90 mole of a monatomic ideal gas is initially
at 285 K and 1 atm.
(a) What is its initial internal energy?
_____ kJ
(b) Find its final internal energy and the work done by the gas
when 420 J of heat are added at constant pressure.
final internal energy ________kJ
work done by the gas _______kJ
(c) Find the same quantities when 420 J of heat are added at
constant volume.
finale internal energy ________kJ
work...

17) Three moles of an ideal monatomic gas expand at a constant
pressure of 2.70 atm ; the volume of the gas changes from 3.10×10−2
m3 to 4.60×10−2 m3 .
Part A
Calculate the initial temperature of the gas.
Part B
Calculate the final temperature of the gas.
Part C
Calculate the amount of work the gas does in expanding.
Part D
Calculate the amount of heat added to the gas.
Part E
Calculate the change in internal energy of...

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.

One mole of ideal gas initially at 300 K is expanded from an
initial pressure of 10 atm to a final pressure of 1 atm. Calculate
ΔU, q, w, ΔH, and the final temperature T2 for this expansion
carried out according to each of the following paths. The heat
capacity of an ideal gas is cV=3R/2.
1. A reversible adiabatic expansion.

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