Question

The gas has a mass of 37.998 g/mol. using the calculated molecular mass, determine the density, in g/l, of this gas at stp, if 1.00 l of this gas effuses through an apparatus in 4.30 min

Answer 1

The density of a gas with a molecular mass of 37.998 g/mol at standard temperature and pressure is 1.696 g/L. This is calculated by dividing the molecular mass by the molar volume of gas at STP, which is 22.4 L/mol.

Step-by-step explanation:

The student has asked to determine the density of a gas at standard temperature and pressure (STP) given its molar mass and the time it takes for 1.00 L of the gas to effuse through an apparatus. To find the density (in g/L) of the gas at STP, we can use the molar mass of the gas and the fact that 1 mole of a gas occupies 22.4 L at STP. The molecular mass of the gas is given as 37.998 g/mol. The density p can be calculated using the equation:

p = \( \frac{molar\ mass}{22.4\ L/mol} \)

Then, substituting the given values:

p = \( \frac{37.998\ g/mol}{22.4\ L/mol} \)

p = 1.696\ g/L

Therefore, the density of the gas is 1.696 g/L at STP.