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We’re being asked to calculate the partial pressure of oxygen in a 7.75 L flask at 65°C.
We will use ideal gas equation to calculate for the pressure:
P = pressure, atm
V = volume, L
n = moles, mol
R = gas constant = 0.08206 (L·atm)/(mol·K)
T = temperature, K
But first, we have to calculate the amount of oxygen (O2) in moles.
Hydrogen and oxygen gas are mixed in a 7.75 L flask at 65°C and contains 0.482 g of hydrogen and 4.98 g of oxygen. What is the partial pressure of oxygen in the flask?
a. 33.5 atm
b. 0.557 atm
c. 67 atm
d. 1.11 atm
e. 0.043 atm
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Based on our data, we think this problem is relevant for Professor Ratliff's class at USF.