Question

For each case determine the change in * entropy for
the surroundings and the universe*, when 1 mole of a
diatomic gas expands from its initial volume of 5 L and 31.5 ◦C
to:

CASE (a) a final volume of 25 L reversibly and isothermically.

CASE (b) irreversibly and isothermically against an external pressure of 1 atm.

CASE (c) a final volume of 25 L reversibly and adiabatically. Yes, it is zero, but you have to demonstrate it.

CASE (d) irreversibly and adiabatically against an external pressure of 1 atm.

*PLEASE, complete answers from CASE A to D.*

Answer #1

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 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)

Calculate the change in entropy for one mole of ideal gas which
expands from an initial volume of 2 L and initial temperature of
500 K to a final volume of 6 L under the following conditions.
P(initial) refers to the pressure when T(initial)= 500K,
V(initial)= 2 L.
a) Irreversible expansion against a constant pressure of
Pinitial/2
b) Irreversible expansion against a vacuum...a 'free
expansion'.
c) Adiabatic irreversible expansion against a constant pressure
of Pfinal
d) Adiabatic reversible expansion

calculate the molar entropy change when (a) water and (b)
benzene are evaporated at their boiling points at a pressure of 1
atm. what are the entropy changes in (i) the system, (ii) the
surroundings, and (iii) the universe, in each case?

Consider an ideal gas enclosed in a 1.00 L container at an
internal pressure of 10.0 atm.
Calculate the work, w, if the gas expands against a constant
external pressure of 1.00 atm to a final volume of 20.0 L.
w=____J
Now calculate the work done if this process is carried out in
two steps.
1. First, let the gas expand against a constant external
pressure of 5.00 atm to a volume of 4.00 L
2. From there, let the...

for the following processes, state whether each of the
thermodynamics quantities, q, w, delta U, and delta H is greater
than, equal to, or less than zero for the system described. Explain
your answers briefly
a) an ideal gas expands adiabaticalally against an external
pressure of 1 bar.
b) an ideal gas expands isothermally against an external
pressure of 1 bar
c) an ideal gas expands adiabatically into a vacuum
d) a liquid at its boiling point is converted reversibly...

A cylinder with a moving piston expands from an initial volume
of 0.250 L against an external pressure of 1.00 atm . The expansion
does 277 J of work on the surroundings. What is the final volume of
the cylinder?

The volume of an ideal gas is adiabatically reduced from 200 L
to 74.3 L. The initial pressure and temperature are 1.00 atm and
300 K. The final pressure is 4.00 atm.
? = 8.314 J/mol.K , ????????? = 1.4, ??????????? = 1.67 and 1
atm = 1.013 × 10^5 Pa. mol.K
(a) Is the gas monatomic or diatomic?
(b) What is the final temperature?
(c) How many moles are in the gas?

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.

The gas inside a cylinder expands against a constant external
pressure of 0.943 atm from a volume of
3.35 L to a volume of 14.40 L. In
doing so, it turns a paddle immersed in 0.951 L of
liquid octane (C8H18).
Calculate the temperature rise of the liquid, assuming no loss of
heat to the surroundings or frictional losses in the mechanism.
Take the density of liquid
C8H18 to be
0.703 g cm-3 and its specific heat to
be 2.22...

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 14 minutes ago

asked 43 minutes ago

asked 45 minutes ago

asked 51 minutes ago

asked 55 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago