A cyclopropane-oxygen mixture is used as an anesthetic. If the partial pressure of cyclopropane in the mixture is 334 mm Hg and the partial pressure of the oxygen is 1.02 atm, what is the total pressure of the mixture in torr?
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Dalton's Law: in a mixture of gases, the total pressure is equal to the sum of partial pressures. Commit that to memory, now. There is a corollary to this law, about the mole ratios, you need to commit that one also. I would be shocked if it is not in your text (Raoult's law)
note the pressures above are in all different units, I suggest changing them all to torr
To find the total pressure of the mixture in torr, we need to convert the given pressures of cyclopropane and oxygen into the same units.
Partial pressure of cyclopropane = 334 mm Hg
Partial pressure of oxygen = 1.02 atm
1 atm is equal to 760 mm Hg (torr). So, we can convert the partial pressure of oxygen to mm Hg by multiplying it by 760:
Partial pressure of oxygen = 1.02 atm x 760 mm Hg/atm = 775.2 mm Hg
Now that we have the pressures of both cyclopropane and oxygen in mm Hg, we can find the total pressure of the mixture by adding them together:
Total pressure = Partial pressure of cyclopropane + Partial pressure of oxygen
Total pressure = 334 mm Hg + 775.2 mm Hg = 1109.2 mm Hg
Therefore, the total pressure of the mixture is 1109.2 mm Hg.