Question

Calculate Δ_{vap}H , the molar enthalpy of vaporization,
of a substance at 338.15 K,

given that its standard enthalpy of vaporization is Δ_{vap}
H^{θ} = 32.45 kJ mol^{−1} vap at 25.0ºC.

The heat capacities are C_{p,m}^{liq} = 46.20 J
K^{−1} mol^{−1} for the liquid and
C_{p,m}^{vap} = 32.20 J K^{−1}
mol^{−1} for the vapor.

Answer #1

At 50.14 K a substance has a vapor pressure of 258.9 torr.
Calculate its heat of vaporization in kJ/mol it if has a vapor
pressure of 161.2 torr at 277.5 K.

Calculate the entropy of vaporization, ΔSvap, for A(l) at 25.0
°C given that the boiling point of A is 72.45 °C, and the molar
heat capacity of A(l) is 116.45 J/(mol·K). Assume that the molar
heat capacity of A(g) is 56.5% of that of A(l).
Calculate the standard Gibbs free energy of vaporization,
ΔG°vap, at 25.0 °C.
Determine the equilibrium constant, K, for the vaporization at
191.0 °C.
Determine the equilibrium constant, K, for the vaporization at
191.0 °C.

a. The standard enthalpy of vaporization of an inorganic
compound is 38.9 kJ/mol. If the temperature at which this phase
change occurs is 221.72 °C, determine ΔS°vap (in
J/mol/K) for this compound. Report your answer to three significant
figures.
b. The entropy of freezing of an organic compound is -21.0
J/mol/K. If ΔH°freez is -14.01 kJ/mol, determine the
temperature (in K) at which this phase change occurs. Report your
answer to two decimal places

Carbon disulfide has a molar enthalpy of vaporization of +29.2
kJmol^-1. At 268 K it has a vapor pressure of 100mmHg. Calculate
the normal temperature of carbon disulfide.

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) 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⋅Krespectively.
A. How much heat is required to convert 40.5
g of ethanol at 36 ∘C to the vapor phase at 78 ∘C?
B. How much heat is required to convert 40.5
g of ethanol at -161 ∘C to...

The normal boiling point of ethanol is 78.3oC. Assuming an
average molar enthalpy of vaporization value of 40.0 kJ/mol in the
temperature interval between 20.0oC and the normal boiling point,
calculate the vapor pressure of ethanol at 30.0oC.

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

1a. From the following vapor
pressure data for octane, an estimate of the molar
heat of vaporization of
C8H18
is kJ/mol.
P, mm Hg
T, Kelvins
100
339
400
377
1b.
The normal boiling point of liquid chloroform
is 334 K. Assuming that its molar heat of
vaporization is constant at 29.9 kJ/mol, the
boiling point of CHCl3 when the
external pressure is 1.34 atm is K.
1c.
The vapor pressure of liquid butanol,
C4H9OH, is
100. mm Hg at 343 K.
A...

Calculate the enthalpy change, ΔH, for the process in
which 10.3 g of water is converted from liquid at 9.4 ∘C to vapor
at 25.0 ∘C .
For water, ΔHvap = 44.0 kJ/mol at 25.0 ∘C and
Cs = 4.18 J/(g⋅∘C) for H2O(l).
How many grams of ice at -24.5 ∘C can be completely converted to
liquid at 9.8 ∘C if the available heat for this process is
5.03×103 kJ ?
For ice, use a specific heat of 2.01 J/(g⋅∘C) and...

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