Question

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?

Answer #1

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?

4. Three moles of a monatomic ideal gas are initially at a
pressure of 1.00 atm and a temperature of 20.0OC. The gas is
compressed adiabatically to a final pressure of 5.00 atm. Find: (a)
the initial volume of the gas; (b) the final volume of the gas; (c)
the final temperature of the gas; (d) the work done by the gas
during the compression.
Answers: (a) 72.1 L; (b) 27.5 L; (c) 285 OC; (d) -97.8
atm-L
Please show...

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 .

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?

An ideal monatomic gas is contained in a vessel of constant
volume 0.330 m3. The initial temperature and pressure of the gas
are 300 K and 5.00 atm, respectively. The goal of this problem is
to find the temperature and pressure of the gas after 24.0 kJ of
thermal energy is supplied to the gas.
(a) Use the ideal gas law and initial conditions to calculate
the number of moles of gas in the vessel. Your response differs
from the...

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?

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.

3. 10.0 moles of ideal gas cloud has an initial pressure of 1.00
bar, initial volume of 100.0L and temperature of 25.0ºC. The cloud
expands adiabatically to a final volume of 1000.0L. Cp,m= 20.79 J /
mol K (Cp,m is molar heat capacity and constant pressure)
a. (10 pts) What is the final pressure of the gas cloud?
b. (10 pts) What is the final temperature of the gas cloud?
c. (10 pts) What is the change in entropy for...

An ideal monatomic gas is contained in a vessel of constant
volume 0.400 m3. The initial temperature and pressure of the gas
are 300 K and 5.00 atm, respectively. The goal of this problem is
to find the temperature and pressure of the gas after 18.0 kJ of
thermal energy is supplied to the gas.
(a) Use the ideal gas law and initial conditions to calculate
the number of moles of gas in the vessel. 80.99 Correct: Your
answer is...

An ideal gas with ? = 1,68 is initially at 4°C in a volume of
9,5 L at a pressure of 1 atm. It is then expanded adiabatically to
a volume of 11,3 L. What is the final temperature (°C ) of the
gas?
Thanks :)

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 4 minutes ago

asked 4 minutes ago

asked 4 minutes ago

asked 7 minutes ago

asked 7 minutes ago

asked 8 minutes ago

asked 8 minutes ago

asked 8 minutes ago

asked 9 minutes ago

asked 10 minutes ago

asked 10 minutes ago

asked 10 minutes ago