3 moles of an ideal gas with 2 atoms under 308 K temperature and
5 atm...
3 moles of an ideal gas with 2 atoms under 308 K temperature and
5 atm are expanded reversible to 1 atm end pressure. Calculate w,
q, ΔU, ΔH values in case of expansion of this expansion by
isothermal and adiabatic way.
If 6.00 moles of a monatomic ideal gas at a temperature of 260 K
are expanded isothermally from a volume of 1.07 L to a volume of
4.61 L .
Calculate the work done by the gas.
Calculate the heat flow into or out of the gas.
If the number of moles is doubled, by what factors do your
answers to parts A and B change?
a) Consider 1.3 moles of an ideal gas at an initial temperature
of 400 K and in a 1.2 m3 closed container. If the gas
goes through an isochoric process to twice the initial temperature,
what is the new pressure of the gas in Pa?
b) Consider 1.3 moles of an ideal gas at an initial temperature
of 400 K and in a 1.2 m3closed container. If the gas
goes through an isothermal process to 3.6 m3, what is
the...
5 moles of ideal gas is initially at 300 K and 5 bar. It is
compressed to 10 bar at 300 K. This change is carried out by two
different reversible processes:
A: heating at constant volume followed by cooling at constant
pressure
B: cooling at constant pressure followed by heating at constant
volume
Depict these processes on a PT graph. (Hand drawn on engineering
sheet would suffice). Calculate ΔU,
ΔH, Q, and W requirements for each path.
Cv=20.78 J/mol.K...
8. Three moles of ideal monatomic gas at 400 K are compressed
from 1 atm to 20 atm. Find for each of the following processes
starting at the same initial condition the work, heat, ΔU, and ΔH
if the compression is performed
a. Isothermally
b. Isochorically
c. Adiabatically
An ideal monatomic gas at an initial temperature of 500 K is
expanded from 5.0 atm to a final pressure of 1.0 atm. Calculate
w, q, DU, and (where applicable)
DH and DT when the expansion is performed (a)
reversibly and isothermally, and (b) reversibly and
adiabatically.
Help Please!!!
5 moles of a monoatomic ideal gas are contained adiabatically at
50 atm pressure and 300 K. The pressure is suddenly released to 10
atm, and the undergoes an irreversible expansion during which it
performs 4000 joules of work. Show to the final temperature of the
gas after the irreversible expansion is greater than that which the
would attain if the expansion from 50 to 10 atm had been conducted
reversibly. Calculate the entropy product as a result of the...
One liter of an ideal monatomic gas (gamma=5/3) at atmospheric
pressure (1.0 atm) and a temperature of 300K is used in the
following cycle: an adiabatic compression to one half its original
volume, followed by a constant-volume cooling to 300K, followed by
an isothermal expansion back to original volume. Determine the work
done by the gas, the heat entering the gas and the change in
thermal energy of the gas in each leg of the cycle. Organize answer
in table....
Ten moles of an ideal gas at 5 bar and 600 K is expanded
adiabatically till its pressure becomes 1/5th the initial pressure.
Then its compressed at constant pressure and finally heated at
constant volume to return to its initial state, calculate: (a) heat
transfer (b) work transfer (c) internal energy and enthalpy change
for each process, and for the entire cycle.Based on the results of
internal energy change and enthalpy change, is the entire process
follows the condition of...
Three moles of an ideal monatomic gas expand at a constant
pressure of 2.40 atm ; the volume of the gas changes from
3.20×10-2 m3 to 4.50×10−2
m3 .
a. Calculate the initial temperature of the gas.
b. Calculate the final temperature of the gas.
c. Calculate the amount of work the gas does in expanding.
d. Calculate the amount of heat added to the gas.
e. Calculate the change in internal energy of the gas.