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What is the pressure, in mm Hg, of 2.50 moles of an ideal gas if it has a volume of 50.0 liters when the temperature is 27.0° C?
Use the ideal gas law: PV=nRT p = pressure v = volume n = number of moles of sample R = ideal gas constant = ~0.08206 (l*atm)/(K*mole) T = Temp in Kelvin
Now we substitute while simultaneously solving for P(pressure) P = (nRT)/V P = (2.50 * 0.08206 * (27+273.15)) / 50 P = Now it's your turn.
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