Question

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). Δ*H*∘fus=7.27kJ/mol

.

Express your answer in joules per kelvin to three significant figures.

Answer #1

The equation for the change in entropy (ΔS) is given below:

where:

n - number of moles

ΔH^{0}_{fus} - molar enthalpy of fusion

T - temperature (melting point)

Given:

n= 4.50 moles

ΔH^{0}_{fus} = 7.27kJ/mol

T = − 116.3 ∘C = (-116.3 + 273.15)K = 156.8 K

Therefore the change in entropy that occurs in the system is:

Hence the change in entropy that occurs in the system
when 4.50 mol of diethyl ether melts at its melting point is
**209 J/K**

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.

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 =

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

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 amount of energy released when 120.0g of diethyl
ether (MW = 74.12 g/mol) is cooled from 53.0 C to 10.0 C ?
boiling point = 26.02 KJ/mol
specific heat capacity, (CH3)2 O(I) 3.74 J/(g.k)
specific heat capacity, (CH3)2 O(g) 2.35 J/(g.k)

Calculate the change in entropy if the number of microstates of
the system changes from 23 to 72. (Give your answer to three
significant figures. Include the sign of the value in your
answer.)
Boltzmann's equation is given below.
ΔS = k * ln (Wfinal/Winitial)
In this equation, ΔS is the change in entropy, Winitial is the
initial number of microstates in the system, Wfinal is the final
number of microstates in the system, and k is Boltzmann's constant,
1.3806503 ...

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

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

he thermodynamic properties for a reaction are related by the
equation that defines the standard free energy, ΔG∘, in
kJ/mol:
ΔG∘=ΔH∘−TΔS∘
where ΔH∘ is the standard enthalpy change in kJ/mol and
ΔS∘ is the standard entropy change in J/(mol⋅K). A good
approximation of the free energy change at other temperatures,
ΔGT, can also be obtained by utilizing this
equation and assuming enthalpy (ΔH∘) and entropy
(ΔS∘) change little with temperature.
Part A
For the reaction of oxygen and nitrogen to...

The standard molar entropy of benzene is 173.3 J/K-mol.
Calculate the change in its standard molar Gibbs energy when
benzene is heated from 25C to 45C.

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