If the temperature of the surroundings is 5.45 °C, calculate the
entropy change (in J/K) for the system (ΔSsys),
surroundings (ΔSsur) and universe
(ΔSuniverse) when 33.6 g of gaseous diethyl ether
(C4H10O) condenses. Report your answers to
two decimal places.
Tfus(°C) | -116.30 |
Tvap(°C) | 34.50 |
ΔH°fus (kJ/mol) | 7.27 |
ΔH°vap (kJ/mol) |
26.52 |
i need these :
1- ΔSsys =
2- ΔSsur =
3 -ΔSuniverse =
We know condensation process is at equilibrium. So its delta G is zero. And so
Delta H = T delta S
We now delta H condensation and temperature. Lets put the number in.
Here Delta H condensation and we are given its delta H of vaporization.
Delta H vap = - delta Hcondensation
Therefore Delta H condensation = - 26.52 x 103 J /mol
Temperature at which condensation occur = 34.50 + 273.15 = 307.65 K
Delta Ssystem = - 26.52 E3 J /mol x 307.65 K= -8158878 J/K mol
We need entropy in J/K
Lets multiply it by number of moles of diethyl ether
Delta Ssystem = -8158878 x (33.6 g / 74.12 g mol-1)
= - 3698574 J/K
DeltaS of surrounding = - q / Tsurr , here surrounding temperature is 5.45 deg C
T = 5.45 + 273.15 = 278.6 k
Delta S surrounding = - 8158878 / 278.6 = 29285.3 J / K
Delta S universe Delta S system + Delta S surrounding = -3698574+29285.3=-3669289 J / K
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