Question

Using the data below - calculate the experimentally determined molar volume of CO2 at STP given the information below:

Lab Temp (T1) = 23.0 Celcius

Lab Pressure (P1) = 76.3 cm HG

Mass of a dry, empty stopped flask (m1) = 82.715g

Mass of the same stopped flask filled with CO2 (m2) = 82.795g

Volume of Water contained by stopped flask (v1) = 144.00 mL

Answer 1

do Labo temperature (Ts) - 23°c Lals pressure (P.) 16.3 cm te g. Mass of dry empty flask (my) - 82.715 gm. Mass of some flaska with filled with CO₂ (m2) = 82.13 Volume of water contained by stopped flaska (V.) = 144.0 mt. Considering density of water agen/ml. at that T. 4P,. volume of covile ta 144.0 mb Mass of co = 162.795 - 82.715) gi 0, 0.08 gm. Molecular weight of coa = 49 gm / ml. 0.08 gm Hence no. of moles in 144.0 ml CO2 z 44 gr/mol am Imol. 20.00182 mol Hence volume of 0.00182 mol o CO2 = 144. ML volume of t mele co a 144 X 10 Lt xt. 0.00182 • 79.121 it, at 23°C & T6- 38cm Assuming co₂ follows ideal gas equation, 2 296K. Now at STP P₂ = 76 cm Hg. Ta ooc 28 273K. Hance volume at STP V₂ - P.V x 12 Tia 23°C 2 (23+273) K 273 it T6.3 X 70 121 12 273 296 x 768 73.26 114 lt So experimentally determined volume of co at STP is 13.26114ht