Asked by Lee
A 1.00 L sample of a pure gas weighs 0.785 g and is at 733.4 torr and 29.2 degree celcius.
a) what is the molar mass of the gas?
b) if the volume of the temperature are kept constant while 0.400 g of the same gas are added to that already in the container, what will the new pressure be?
a) what is the molar mass of the gas?
b) if the volume of the temperature are kept constant while 0.400 g of the same gas are added to that already in the container, what will the new pressure be?
Answers
Answered by
DrBob222
Note the correct spelling of celsius.
1). Use PV = nRT and solve for n = number of moles, then n = grams/molar mass. You have n and grams, solve for molar mass. Don't forget to convert T to kelvin and P to atmospheres.
2) Add 0.400 g to grams already there, use the molar mass from the first part to convert grams to moles, then use PV = nRT and solve for pressure in atmospheres.
1). Use PV = nRT and solve for n = number of moles, then n = grams/molar mass. You have n and grams, solve for molar mass. Don't forget to convert T to kelvin and P to atmospheres.
2) Add 0.400 g to grams already there, use the molar mass from the first part to convert grams to moles, then use PV = nRT and solve for pressure in atmospheres.
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