Question

One mole of an ideal gas initially at a temperature of
*T*_{i} = 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
*T*_{f} of the gas.

K

(b) Calculate the work done *on* the gas during the
expansion.

kJ

Answer #1

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

A cylinder with a moveable piston on top, free to move up and
down, contains one mole of an ideal gas initially at a temperature
of Ti = 3.8°C. The cylinder is heated at a constant pressure of
1.00 atm, and it expands to seven times its original volume. (a)
Calculate the new temperature Tf of the gas (in K). (No Response) K
(b) Calculate the work done (in kJ) on the gas during the
expansion.

A sample consisting of 2.5 moles of ideal gas (Cp,m
=20.8 J/K) is initially at 3.25 atm and 300 K. It undergoes
reversible adiabatic expansion until its pressure reaches 2.5 atm.
Calculate the final volume, the final temperature, and the work
done.

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...

An ideal gas initially at 350 K undergoes an isobaric expansion
at 2.50 kPa. The volume increases from 1.00 m3 to 3.00 m3 and 13.0
kJ is transferred to the gas by heat. (a) What is the change in
internal energy of the gas? kJ (b) What is the final temperature of
the gas?

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 initially at temperature T0 reversibly
expands from volume V0 to 2V0,
(a) at constant temperature (b) at constant pressure.
Calculate the work, the heat, and change in internal energy of
the gas in each process.

2.)1.0 mol sample of an ideal monatomic gas originally at a
pressure of 1 atm undergoes a 3-step process as follows:
(i) It expands
adiabatically from T1 = 588 K to T2 = 389 K
(ii) It is compressed at
constant pressure until its temperature reaches T3 K
(iii) It then returns to its
original pressure and temperature by a constant volume process.
A). Plot these processes on a PV diagram
B). Determine the temperature T3
C)....

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 vessel with a movable piston contains 1.90 mol of an ideal gas
with initial pressure
Pi = 2.03 ✕ 105 Pa,
initial volume
Vi = 1.00 ✕ 10−2
m3,
and initial temperature
Ti = 128 K.
(a) What is the work done on the gas during a constant-pressure
compression, after which the final volume of the gas is 2.50
L?
J
(b) What is the work done on the gas during an isothermal
compression, after which the final pressure...

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