What is the volume occupied by 0.17 grams of gaseous H2S at 27◦C and 380 torr?

Question

What is the volume occupied by 0.17 grams of gaseous H2S at 27◦C and 380 torr?

Answer 1

First find moles of gas: (0.17g H₂S) * (1 mol H₂S /34.1g H₂S) = 0.0049₉ mole (3rd digit is kept for precision but is not significant). Then use ideal gas law PV = nRT, yielding

V = nRT/P = (0.0049₉ mol) (62.36 L torr/mole K) (27 + 273K) / (380 torr) = 24.5 L ≅ 25 L to 2 sig figs.

Answer 2

Remember to convert from Torr to atm. Watch this, it'll help.

https://youtu.be/2spz4y7iTBs