Question

One mole of an ideal monatomic gas is compressed irreversibly from 2.00 atmto 6.00 atmwhile being cooled from 400. K to 300. K. Calculate ?U, ?H, and ?S for this process.

Answer #1

For an ideal gas

At step 1

For isothermal process

Change in internal energy H = U = 0

Entropy change

= 1 mol x 8.314 J/mol·K x ln (2/6)

= - 9.130 J/K

At step 2

Change in enthalpy

= (5/2) x 1 mol x 8.314 J/mol·K x (300 - 400)K

= - 2.08 x 10^3 J

Change in internal energy

= - 2.08 x 10^3 J - 1 mol x 8.314 J/mol·K x (300 - 400)K

= - 1.25 x 10^3 J

Change in entropy

= (5/2) x 1 mol x 8.314 J/mol·K x ln ( 300/400)

= - 5.98 J/K

For combined process

Change in enthalpy

H = H for step1 - H for step 2

= 0 - 2.08*10^3 J

= 2.08 x 10^3 J

Change in internal energy

U = U for step1 - H for step 2

= 0 - 1.25 x 10^3

= - 1.25 x 10^3 J

Change in entropy

S = S for step1 - S for step 2

= - 9.130 - 5.98

= - 15.1 J/K

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.

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)

A mole of a monatomic ideal gas is taken from an initial
pressure p and volume V to a final pressure 3p and volume 3V by two
different processes: (I) It expands isothermally until its volume
is tripled, and then its pressure is increased at constant volume
to the final pressure. (II) It is compressed isothermally until its
pressure is tripled, and then its volume is increased at constant
pressure to the final volume. Show the path of each process...

A tank contains one kilomole of a monatomic ideal gas, argon,
and has a pressure of 1 atm and a temperature of 300 K. The mass of
an argon atom is 6.63 x 10-26 kg.
a.) Calculate the internal energy, U, of the gas in Joules.
b.) Calculate the average energy per atom in eV. (1eV = 1.602 x
10-19 J)
c.) Calculate the partition function, Z.
d.) Calculate the entropy of the assembly, S

Consider the adiabatic, reversible expansion of a closed 1 mole
sample of monatomic ideal gas from P1 = 100 bar, V1 = 1dm3, and T1
= 1200K to V2 = 1.5 dm3.
What is the final temperature of the gas? What are the values of
ΔE, ΔS and w for the process described in the previous question? ΔE
= kJ ΔS = J/K w = kJ

One-third mole of a monatomic ideal gas expands adiabatically
and does 640 J of work. By how many kelvins does its temperature
change? K
Specify whether the change is an increase or a decrease.

Assume that one mole of a monatomic (CV,m = 2.5R) ideal gas
undergoes a reversible isobaric expansion at 1 bar and the volume
increases from 0.5 L to 1 L. (a) Find the heat per mole, the work
per mole done, and the change in the molar internal energy, ΔUm,
the molar enthalpy, ΔHm, for this process. b) What are the entropy
changes ΔSm of the system and of the surroundings? Is this process
spontaneous? Justify your answer.

One mole of an ideal gas at 300 K is expanded adiabatically and
reversibly from 20 atm to 1 atm. What is the final temperature of
the gas, assuming Cv= 3/2R.
Question 1 options: a) 400 K b) 250 K c)156 K d)90.5 K

1 mole of a non-ideal gas is compressed isothermally at 100°C
from 1 bar to 50 bar. What are the heat and work needed for this
(reversible) compression if the gas conforms to the principle of
corresponding states?
The critical properties of the non-ideal gas are Tc = 406 K
and Pc = 11.3 MPa.

2.00-mol of a monatomic ideal gas goes from State A to State D
via the path A→B→C→D:
State A PA=11.0atm, VA=13.00L
State B PB=11.0atm, VB=6.50L
State C PC=20.5atm, VC=6.50L
State D PD=20.5atm, VD=22.00L
Assume that the external pressure is constant during each step
and equals the final pressure of the gas for that step.
Calculate q for this process.
Calculate w for this process.

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 2 minutes ago

asked 2 minutes ago

asked 3 minutes ago

asked 4 minutes ago

asked 4 minutes ago

asked 4 minutes ago

asked 4 minutes ago

asked 4 minutes ago

asked 9 minutes ago

asked 9 minutes ago

asked 14 minutes ago

asked 15 minutes ago