The partial pressure of O₂ from daniel's 2.5L bottle that contains a mixture of O₂, N₂ and CO₂ under a total pressure of 5.10 atm is 2.171atm.
<h3>What is partial pressure? </h3>
In a mixture of gases, each constituent gas has a partial pressure which is the notional pressure of that constituent gas as if it alone occupied the entire volume of the original mixture at the same temperature.
How to calculate the partial pressure of O₂?
Volume (V) = 2.5L
T = 273K
o₂ + N₂ + CO₂ ---> Total pressure P = 5.1atm
N₂ = 0.31 mol
Partial pressure CO₂ = 0.25atm
R = 0.0821L (ideal gas constant with given volume in L and temperature in K)
P*V = n*R*T
n = P*V / R*T
= (5.1 * 2.5) / (0.0821 * 273)
= 12.75 / 22.4133
= 0.56886 mole
Partial pressure of N₂
= mol fraction * Total pressure
= (0.31 / 0.56886) * 5.1
= 2.779atm
Total pressure
P = P O₂ + P N₂ + P CO₂
5.2 = P O₂ + 2.779 + 0.25
P O₂ = 5.2 - 2.779 - 0.25
P O₂ = 2.171atm
Therefore, the partial pressure of O₂ is 2.171atm.
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