Assume that you take a flask, evacuate it to remove all the air, and find its ma

Question

Assume that you take a flask, evacuate it to remove all the air, and find its mass to be 499.7g . You then fill the flask with argon to a pressure of 2.50atm and reweigh it.
What would the balance read (in grams) if the flask has a volume of 8.60L  and the temperature is 18.0?C?          Assume that you take a flask, evacuate it to remove all the air, and find its mass to be 499.7g . You then fill the flask with argon to a pressure of 2.50atm and reweigh it. Assume that you take a flask, evacuate it to remove all the air, and find its mass to be 499.7g . You then fill the flask with argon to a pressure of 2.50atm and reweigh it. Assume that you take a flask, evacuate it to remove all the air, and find its mass to be 499.7g . You then fill the flask with argon to a pressure of 2.50atm and reweigh it.
What would the balance read (in grams) if the flask has a volume of 8.60L  and the temperature is 18.0?C?         

Explanation / Answer

Ideal gas equation: PV = nRT

Moles of Ar = n = PV/RT

= 2.50 x 8.60/(0.08206 x (273.15 + 18.0)) = 0.8999 mol


Mass of Ar = moles x molar mass of Ar

= 0.8998 x 39.95 = 35.95 g


Balance reading = mass of flask + mass of Ar

= 499.7 + 35.95

= 535.65 g = 535.7 g

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