a) Calculate the density in g/L of the vapor of your unknown at experimental tem
ID: 993159 • Letter: A
Question
a) Calculate the density in g/L of the vapor of your unknown at experimental temperature and pressure.
b) What would the density of the apor of your unknown be at STP assuming that it existed as a vapor at these conditions?
Below is the data obtained from the lab. The molecular formula of the unknown is : C6H12
Please show all work!
Flask 1 Weight of Flask, Foil Cap and Condensed Liquid 79.88%, Weight of Empty Flask with Foil | Weight of ' . 5qu Condensed Liquid,54 Temperature of Vapor (oC) Temperature of Vapor (K) °C+ 273, 15 373.15K Pressure 759.9lo8 mmHa .99995 78 Volume of Flask 10.152 Moles of Vapor 10.00 910 !09.( Molar Mass of Liquid 3 VAg Percent Error OF MOLAR 19 % MAExplanation / Answer
pressure (p) = 0.999 atm
T = 100 C = 100 + 273 = 373 K
moles (n) = 0.00496
Volume = 0.152 L
According to Ideal gass equation PV =nRT, n = number of moles
For the compound C6H12 molecular weight = 84
Percentagr error = absolute value x100 / Theoritical value
percentage error = 19
19 = m x 100 / 84
absolute value(m) = 84 x 19/100
m = 15.96
then the value is = 84- 15.96 = 68.04
PV =nRT , R = 0.0821 L atm K-1 mol-1
0.999 x 0.152 = wt/68.04 x 0.0821 x 373
0.1518 = wt/68.04 x 30.623
wt / 84 = 0.00495
wt = 0.00495 x 68.04
wt = 0.336 g.
dencity (d) = m / V
d = 0.336/0.152
d = 2.215 g/L.
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