Question

One mole of an ideal gas with is compressed adiabatically in a single stage with a constant opposing pressure equal to 10atm. pressure is 10 atm. Calculate the final temperature of the gas, w, q, ΔU and ΔH. HINT – this is not reversible expansion.

Answer #1

a) **Heat, Q**

Since its an adiabatic process, there is no trnafer of heat, therefore q = 0.

b) **Final temperature**

Assumption monoatomic gas

= 5/3

Intial T = 273 K, Initiial P = 1 bar (Since 1 mole of ideal at standard temperature & pressure)

Final P = 10 atm = 10.1325 bar, Final Temp = T

**For adiabatic process**

P^{-2/3}T^{5/3} = constant

1^{-2/3}(273)5/3=
(10.1325)^{-2/3}T^{5/3}

T = 689.36 K

c) **Change in Internal Energy**

= degrees of freedom/ 2 = 3/2 = 1.5

n = 1

= 689.36 - 273 = 416.36 K

= 1.5*8.314*416.36 = 5192.42 J

d) **Work**

Here Q = 0

= - 5192.42 J

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.

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)

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.

Solve the following:
a) Calculate ΔU for the irreversible isothermal compression of 1
mole of ideal gas at 290 K from an initial pressure of 3.2 KPa to a
final pressure of 46 kPa by an constant external pressure of 46
kPa. Give your answer in kilojoules.
b) Consider a reversible isothermal expansion (or compression)
of 4.0 mole(s) of an ideal gas at 28°C from 6.5 atm to 3.0 atm.
Calculate the amount of heat transferred to the system in...

One mole of an ideal gas
CP=7R2 in a closed
piston/cylinder arrangement is compressed from
Ti=200 K , Pi=0.5
MPa to Pf=5 MPa by following
paths:.
ADIABATIC path
ISOTHERMAL path
Calculate ΔU, ΔH, Q and WEC for both paths.
NOTE: Keep the answers in terms of ‘R’.

State whether the following are reversible processes. Explain
your reasoning.
(a.) One mole of (ideal) diatomic gas is compressed from 200 cm3
to 100 cm3 at a constant pressure of 100 kPa.
(b.) One mole of (ideal) diatomic gas is adiabatically
compressed from 200 cm3 to 100 cm3.

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

A two mole sample of an ideal diatomic gas expands
slowly and adiabatically from a pressure of 5 atm. and a volume of
10 liters up to a final volume of 30 liters.
a) What is the final pressure of the gas ?,
b) Whatis the heat, work and internal energy?

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

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 3 minutes ago

asked 4 minutes ago

asked 25 minutes ago

asked 38 minutes ago

asked 38 minutes ago

asked 42 minutes ago

asked 46 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 2 hours ago

asked 2 hours ago