Question

Calculate the entropy of fusion of a compound at 25°C given
that

its enthalpy of fusion is 32 kJ mol−1 at its melting point of
146°C and

the molar heat capacities (at constant pressure) of the liquid
and solid

forms are 28 J K−1 mol−1 and 19 J K−1 mol−1,
respectively.

Answer #1

Calculate the entropy of fusion of a compound at 25°C given
that
its enthalpy of fusion is 32 kJ mol−1 at its melting point of
146°C and
the molar heat capacities (at constant pressure) of the liquid
and solid
forms are 28 J K−1 mol−1 and 19 J K−1 mol−1,
respectively.

A piece of solid antimony weighing
34.3 g at a temperature of 618 °C
is placed in 343 g of liquid
antimony at a temperature of 754
°C. After a while, the solid melts and a completely liquid sample
remains. Calculate the temperature after thermal equilibrium is
reached, assuming no heat loss to the surroundings.
The enthalpy of fusion of solid antimony is
ΔHfus = 19.6 kJ/mol at its melting
point of 631 °C, and the molar heat capacities for...

A piece of solid lead weighing
45.3 g at a temperature of 308 °C
is placed in 453 g of liquid lead
at a temperature of 374 °C. After a while, the
solid melts and a completely liquid sample remains. Calculate the
temperature after thermal equilibrium is reached, assuming no heat
loss to the surroundings.
The enthalpy of fusion of solid lead is
ΔHfus = 4.77 kJ/mol at its melting
point of 328 °C, and the molar heat capacities for...

A piece of solid lead weighing
43.2 g at a temperature of 314 °C
is placed in 432 g of liquid lead
at a temperature of 367 °C. After a while, the
solid melts and a completely liquid sample remains. Calculate the
temperature after thermal equilibrium is reached, assuming no heat
loss to the surroundings.
The enthalpy of fusion of solid lead is
ΔHfus = 4.77 kJ/mol at its melting
point of 328 °C, and the molar heat capacities for...

Ethanol (C2H5OH) melts at -114 °C. The enthalpy of fusion is
5.02 kJ/mol. The specific heats of solid and liquid ethanol are
0.97 J/g•K and 2.3 J/g•K, respectively. How much heat (kJ) is
needed to convert 25.0 g of solid ethanol at -125 °C to liquid
ethanol at -40 °C

Ethanol (C2H5OH) melts at -114 ∘C and boils at 78 ∘C. The
enthalpy of fusion of ethanol is 5.02 kJ/mol, and its enthalpy of
vaporization is 38.56 kJ/mol. The specific heat of solid and liquid
ethanol are 0.97 J/g⋅K are 2.3 J/g⋅K respectively. Q: A) How much
heat is required to convert 36.5 g of ethanol at 35 ∘C to the vapor
phase at 78 ∘C? B) How much heat is required to convert 36.5 g of
ethanol at -167...

Ethanol, C2H5OH, (MW 46.06 g/mol) melts at
-114 °C. The enthalpy of fusion is 5.02 kJ/mol. The specific heats
of solid and liquid ethanol are 0.97 J/g-K and 2.3 J/g-K,
respectively. How much heat (kJ) is needed to convert 20.0 g of
solid ethanol at -135 °C to liquid ethanol at -50 °C?
please show work

The enthalpy of fusion for Lauric acid (C12H24O2) is 32.86
kJ/mol and enthalpy of vaporization is 63.82 kJ/mol. The melting
point is 43.2 degrees C. How much heat is absorbed to raise the
temperature of a 0.650g sample from 22.0 degrees C to 56.3 degrees
C? The heat capacity of the solid is 2.15 J/g degrees C and the
heat capacity of the liquid is 3.62 J/g degrees C

Ethanol (C2H5OH) melts at -114 °C. The enthalpy of fusion is
5.02 kJ/mol. The specific heats of solid and liquid ethanol are
0.97 J/g-K and 2.3 J/g-K, respectively. How much heat (kJ) is
needed to convert 25.0 g of solid ethanol at -135 °C to liquid
ethanol at -60 °C?
A. 207.3
B. -13.3
C. 6.34
D. 3617
E. 8.63

Calculate ΔvapH , the molar enthalpy of vaporization,
of a substance at 338.15 K,
given that its standard enthalpy of vaporization is Δvap
Hθ = 32.45 kJ mol−1 vap at 25.0ºC.
The heat capacities are Cp,mliq = 46.20 J
K−1 mol−1 for the liquid and
Cp,mvap = 32.20 J K−1
mol−1 for the vapor.

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