How much volume in liters will 100.0 grams of oxygen occupy at 100 degrees celcius and 100 atm pressure?
Use PV = nRT
Don't forget to use T in Kelvin.
Post your work if you have trouble.
The above posted by DrBob222.
To determine the volume in liters that 100.0 grams of oxygen will occupy at 100 degrees Celsius and 100 atm pressure, we can use the ideal gas law equation:
PV = nRT
where:
P is the pressure (in atm)
V is the volume (in liters)
n is the number of moles of gas
R is the ideal gas constant (0.0821 L·atm/(mol·K))
T is the temperature (in Kelvin)
First, we need to convert the given temperature from Celsius to Kelvin:
T(K) = T(C) + 273.15
T(K) = 100 + 273.15
T(K) = 373.15 K
Next, we need to calculate the number of moles of oxygen by using its molar mass. The molar mass of oxygen (O₂) is 32.00 g/mol. To convert grams to moles, we can use the equation:
n = m / M
where:
n is the number of moles
m is the mass (in grams)
M is the molar mass (in g/mol)
n = 100.0 g / 32.00 g/mol
n = 3.125 mol
Now we have all the necessary values, so we can plug them into the ideal gas law equation to solve for the volume:
PV = nRT
(100 atm) * V = (3.125 mol) * (0.0821 L·atm/(mol·K)) * (373.15 K)
Simplifying the equation:
100V = 1237.17 L·atm
V = 1237.17 L·atm / 100
V = 12.37 liters
Therefore, 100.0 grams of oxygen will occupy approximately 12.37 liters at 100 degrees Celsius and 100 atm pressure.