section a and b please full procedure, thank you
(a). Vapour pressure of a liquid at its normal boiling point is equal to 1 atm (that is atmospheric pressure).
So, we can take P1 = 1.00 atm, T1 = - 29.2 0C = (273.15 − 29.2) K = 243.95 K,
T2 = 105 0F = (105°F − 32) × 5/9 + 273.15= 313.706 K, P2 = ?
Using Clausius Clapeyron equation:
ln (P2 / P1) = (vapH° / R) X (1/T1 - 1/T2)
ln (P2 / P1) = (20250 J mol-1 / 8.3145 J K-1 mol-1) X (1/243.95 K - 1/313.706 K)
ln (P2 / P1) = (2435.504 K) X (0.0041 - 0.0032) K-1 = 2435.504 X 0.0009
ln (P2 / P1) = 2.1919 (P2 / P1) = e2.1919 = 8.9522
P2 = 8.9522 X 1 atm = 8.9522 atm
(b) Change in molar volume = V = 0.517 cm3/mol = 5.17 X 10-7 m3/mol, T = 234.3 K, Fus H = 2.292 kJ/mol
Pressure = h ρ g
where h= height od the column = 15 m, ρ = density = 13.6 g/cm3 = 13600 kg/ m3 , g = 9.8 ms-2 = 9.8 N kg-1
So, P2 = 15 m X 13600 kg/ m3 X 9.8 N kg-1 = 1999200 Pa = 1999.2 kPa
P1 = 1 atm = 101.325 kPa
P = 1999.2 kPa - 101.325 kPa = 1897.875 kPa
Using Clapeyron Equation:
T = (T V P) / Fus H
T = (234.3 K X 5.17 X 10-7 m3/mol X 1897.875 kPa) / 2.292 kJ mol-1
T = (0.2299/ 2.292 ) K = 0.1003 K
T2 = T1 + T = 234.3 K + 0.1003 K = 234.4003 K
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section a and b please full procedure, thank you 1) We'll start with a pair of...
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