A closed 5.00 L container is filled with a mixture of 4.00 moles of hydrogen gas, 8.00 moles of oxygen, 12.0 moles of helium, an d 6.00 moles of nitrogen. What is the pressure due to the oxygen in this container at a temperature of 25 °C?
1 answer:
Answer:
24.44 atm
Explanation:
Considering that this gas mixture behaves like an ideal gass, and that all component gases are ideal gases, we can use:
PV=nRT
Then:
P=nRT/V
Where:
n= N° of moles
R= gas constant= 0.082 Lt*atm/K*mol
T= temperature (in Kelvin)
V = volume (in Lt)
Finally, statement says:
T = 25°C = 298 K
V = 5 Lt
n = 8 moles (for O₂)
P = [8 molx(0.082 Lt*atm/K*mol)x298 K]/5 Lt
P = 24.44 atm would be the pressure due to O₂ (partial pressure of the oxygen)
You might be interested in
Answer:
Nucleic acids
That make our genes.
Answer:sulfer by itself is not pleasant and it can be dangerous by itself but in large amounts.
Explanation:
Formula for calculation of neutrons is Mass number - atomic number, here values are given. By putting values in formula 76-35= 41. Number of neutrons 41
The atomic number, the number of protons and the number of electrons.
Pv=nRT
