Question

What is the mass of 50 cc of carbon monoxide at STP?

Answer 1

Using the ideal gas law: PV=nRT where

P is in atms, V is in liters, n is moles, R is the universal gas constant of 0.082056 and

T is absolute or Kelvin

STP is defined as P = 1 atm, T = 273 degrees K

Thus: (1 atm) (12ml/1000 ml/l) = n moles (0.082056)(273 degrees)

n = 1 (12) / (0.082056)(273) = 0.0005356 moles

Hydrogen exists as a diatomic molecule, atomic weight of hydrogen is 1, thus a mole of hydrogen gas weighs 2 grams.

Thus mass of 12 cc Hydrogen gas at STP =

2 grs/mole (0.0005356moles)= 0.0010712 g = 1.0712 x 10^-3 g

There is no such thing as a true ideal gas and there are rounding errors in the value of R so other answers may be different but close.

A prior answer uses the density of hydrogen at STP and, if this density is known to you, that is a great way to answer this question. Not knowing the density, use the ideal gas law.

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