To find the partial pressure of oxygen in the flask, we first need to calculate the moles of each gas present in the flask.
1. Calculate moles of hydrogen:
moles of hydrogen = mass of hydrogen / molar mass of hydrogen
moles of hydrogen = 0.482 g / 2.016 g/mol = 0.239 moles
2. Calculate moles of oxygen:
moles of oxygen = mass of oxygen / molar mass of oxygen
moles of oxygen = 4.98 g / 32.00 g/mol = 0.156 moles
3. Now, we can use the ideal gas law to calculate the partial pressure of oxygen:
PV = nRT
where:
P = partial pressure of oxygen
V = volume of the flask in liters (7.75 L)
n = moles of oxygen (0.156 moles)
R = ideal gas constant (0.0821 L.atm/mol.K)
T = temperature in Kelvin (65 + 273 = 338 K)
Substitute the values into the equation:
P * 7.75 = 0.156 * 0.0821 * 338
P * 7.75 = 4.1888
P = 4.1888 / 7.75
P ≈ 0.54 atm
Therefore, the partial pressure of oxygen in the flask is approximately 0.54 atm.
Hydrogen and oxygen gas are mixed in a 7.75 L flask at 65oC and contains 0.482 g of hydrogen and 4.98 g of oxygen. What is the partial pressure of oxygen in the flask?
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