1.) 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, and 6.00 moles of nitrogen. What is the pressure in this container at a temperature of 25 °C?
2.) 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, and 6.00 moles of nitrogen. What is the pressure due to the oxygen in this container at a temperature of 25 °C?
Please explain, Thank you~
(30(.08206)(298))/5
P=(ntotal(RT))/R
=147atm
for number two do the same but with 8 instead of 30
total moles=30moles
PV=nRT solve for P, change temps to K
b.Aren't these the same question?
(30(.08206)(298))/5
P=(ntotal(RT))/R
=147atm
for number two do the same but with 8 instead of 30
because it is only the oxygen
To find the pressure in the container, we can use the ideal gas law equation: PV = nRT.
1.) To find the pressure in the container, we need to calculate the total moles of gas in the mixture first. The total moles of gas is the sum of the individual mole amounts of each gas.
Total moles of gas = 4.00 moles (hydrogen) + 8.00 moles (oxygen) + 12.0 moles (helium) + 6.00 moles (nitrogen) = 30.0 moles
Next, we need to convert the temperature to Kelvin since the ideal gas law equation uses Kelvin temperature scale.
Temperature in Kelvin = 25 °C + 273.15 = 298.15 K
Now we can plug in the values into the ideal gas law equation:
PV = nRT
P(5.00 L) = (30.0 moles)(0.0821 L·atm/K·mol)(298.15 K)
Now we can solve for P (pressure):
P = (30.0 moles)(0.0821 L·atm/K·mol)(298.15 K) / 5.00 L
P = 147.85 atm
Therefore, the pressure in the container at a temperature of 25 °C is approximately 147.85 atm.
2.) To find the pressure only due to the oxygen gas in the container, we can use the same equation but with the mole amount of only oxygen gas.
P(5.00 L) = (8.00 moles)(0.0821 L·atm/K·mol)(298.15 K) / 5.00 L
P = 39.54 atm
Therefore, the pressure due to the oxygen gas in the container at a temperature of 25 °C is approximately 39.54 atm.