Question

An
ideal monatomic gas at 405 K expands adiabatically and reversibly
to three times its volume. What is its final temperature (in
K)?

Answer #1

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.

2.50 mol of a diatomic ideal gas expands adiabatically and
quasi-statically. The initial temperature of the gas is 325 K. The
work done by the gas during expansion is 7.50 kJ.
(a) What is the final temperature of the gas?
K
(b) Compare your result to the result you would get if the gas
were monatomic. (Calculate the final temperature if the gas were
monatomic.)
K

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

The volume of a monatomic ideal gas doubles in an adiabatic
expansion.
Considering 115 moles of gas with an initial pressure of 350 kPa
and an initial volume of 1.4 m3 . Find the pressure of the gas
after it expands adiabatically to a volume of 2.8 m3 .
Pf= 110 kPa
Find the temperature of the gas after it expands adiabatically
to a volume of 2.8 m3 .

The volume of an ideal gas is adiabatically reduced from 217 L
to 65.6 L. The initial pressure and temperature are 1.70 atm and
300 K. The final pressure is 9.07 atm. (a) Is the
gas monatomic, diatomic, or polyatomic? (b) What
is the final temperature? (c) How many moles are
in the gas?

1. An ideal monatomic gas, with 24.05 moles, expands
adiabatically from 0.500m^3 to 1.75 m^3. IF the initial pressure
and temperature are 1.40x10^5 Pa and 350K, respectively, find the
change in internal energy of the gas if the final temperature of
the gas is 152K.
2. A fridge does 17.5 KJ of work while moving 120KJ of thermal
energy from inside the fridge. Calculate the fridge's coefficient
of performance.

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?

An ideal gas with γ = 1.400 expands adiabatically from a
pressure of 365.0 Pa and a volume of 70.00 m3 , doing 101.0 J of
work while expanding to a final volume. What is its final
pressure-volume product?

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.

A 2.00-mol sample of a diatomic ideal gas expands slowly and
adiabatically from a pressure of 5.04 atm and a volume of 13.0 L to
a final volume of 31.0 L.
(a) What is the final pressure of the gas?
atm
(b) What are the initial and final temperatures?
initial
K
final
K
(c) Find Q for the gas during this process.
kJ
(d) Find ΔEint for the gas during this
process.
kJ
(e) Find W for the gas during...

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