Question

Part A Calculate the change in entropy that occurs in the system when 56.7 g of water vaporizes from a liquid to a gas at its boiling point (100.0?C). ?H?vap = 40.7 kJ/mol Express your answer to three significant figures.

Answer #1

Calculate the change in entropy that occurs in the system when
4.50 mol of diethyl ether (C4H10O) melts at its melting point (−
116.3 ∘C). ΔH∘fus=7.27kJ/mol
.
Express your answer in joules per kelvin to three significant
figures.

Calculate the change in entropy of the surroundings when 1.0 mol
of water vaporizes as 1000C. The heat of vaporization of
water is 40.6 kj/mol

If the temperature of the surroundings is -244.32 °C, calculate
the entropy change (in J/K) for the system (ΔSsys), surroundings
(ΔSsur) and universe (ΔSuniverse) when 40.4 g of liquid oxygen (O2)
freezes. Report your answers to two decimal places. Tfus(°C)
-218.79 Tvap(°C) -182.96 ΔH°fus (kJ/mol) 0.44 ΔH°vap (kJ/mol)
6.82

For water ∆H°vap = 40.7 kJ/mol at 100.°C, its boiling point.
Calculate w and ∆E for the vaporization of 1.00 mol water at 100.°C
and 1.00 atm pressure.

If the temperature of the surroundings is 38.36 °C, calculate
the entropy change (in J/K) for the system (ΔSsys), surroundings
(ΔSsur) and universe (ΔSuniverse) when 48.1 g of gaseous carbon
tetrachloride (CCl4) condenses. Report your answers to two decimal
places.
Tfus(°C) -23.00
Tvap(°C) 76.80
ΔH°fus (kJ/mol) 3.28
ΔH°vap (kJ/mol) 29.82

Calculate the enthalpy change, ΔH, for the process in which 14.3
g of water is converted from liquid at 4.0 ∘C to vapour at 25.0 ∘C
. For water, ΔvapH = 44.0 kJ mol−1 at 25.0 ∘C and Cs = 4.18 J g−1
∘C−1 for H2O(l). Express your answer to three significant figures
and include the appropriate units.

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 =

Calculate the amount of heat ( in kJ) required to convert 344.0
g of liquid water at 22.5 oC into steam at 145.0
°C. ( Heat of vaporization of water at its boiling
point = 40.7 kJ/mol., specific heats of water and steam are 4.184
J/g °C and 2.01 J/g °C,
respectively. )

Part A
Calculate the enthalpy change, ΔH, for the process in
which 44.0 g of water is converted from liquid at 7.6 ∘C to vapor
at 25.0 ∘C .
For water, ΔHvap = 44.0 kJ/mol at 25.0 ∘C and
s = 4.18 J/(g⋅∘C) for H2O(l)
Express your answer numerically in kilojoules.
Part B
How many grams of ice at -11.0 ∘C can be completely converted to
liquid at 9.4 ∘C if the available heat for this process is
5.66×103 kJ...

Calculate the change in entropy of the system when 15.0g of ice
at -12.0C is converted to water vapor at 105C at a constant
pressure of 1bar. The constant pressure molar heat capacity ofH2O
(s) and H2O (l) is 75.291J/mol K and that of H2O (g) is 33.58 J/K
mol

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