Density of an Ideal Gas?

Question

Assuming ideal gas behaviour, what would be the density of gaseous chlorine (Cl2) at 22 °C and 774 mmHg?

Answer 1

From the state equation of the ideal gases: p*V = n*R*T, substituting n = m/Mr (where Mr the molar mass) and m = d*V, you get:

p*V = d*V*R*T/Mr, so:

d = p*Mr/R*T

Now p = 774/760 atm, Mr = 71 for Cl2, R = 0.082 L*atm/mol*K, T = 22 + 273 = 295 K and:

d = 774*71/760*0.082*295 = 2.989 g/L or 3 g/L approx.

Answer 2

you will discover the traditional quantity for one mole of gas molecules. the quantity is typical because of the fact one mole of atoms or molecules in vapor area (a gas) aways takes up the comparable quantity at STP in spite of what style of atoms/molecules they are (a minimum of they do in the event that they are "appropriate"). So, that provides you with the quantity. The molecular weight components the mass of that quantity of gas so which you will calculate density (grams consistent with cubic centimeter) for N2O at STP. because of the fact it quite is appropriate gas, you need to use PV=nRT to discover the quantity at 24C and 747 mmHg. that provides you with a clean quantity and you have not won or lost any mass so which you will calculate a clean density. stable luck