Question

In a closed container, one gram of water (1 cm^{3}) is
boiled under constant pressure of 1 atm (1.013 × 10^{5} Pa)
until it changes into steam.

The heat of vaporization at this pressure is L_{v} =
2.256 × 10^{6} J/kg = 2256 J/g.

Assume that water vapor behaves like an ideal gas. The
temperature of the steam is 373 K, number of moles of water vapor n
= 0.0546 (g mol), the ideal gas constant R = 82.057
(cm^{3}·atm/g mol·K).

(a) How much volume (in cm^{3}) of steam is
produced?

(b) How much work is done by the water when it vaporizes?

(c) How much has the internal energy increased?

Answer #1

4.7 cm3 of water is boiled at atmospheric pressure to become
4063.2 cm3 of steam, also at atmospheric pressure.
1. Calculate the work done by the gas during this process. The
latent heat of vaporization of water is 2.26 × 106 J/kg . Answer in
units of J.
2. Find the amount of heat added to the water to accomplish this
process. Answer in units of J.
3. Find the change in internal energy. Answer in units of J.

A 2.0 L-closed container at 300 K holds 100 cm3 of
H2O(l). The equilibrium vapor pressure is found to be
0.0328 atm. What pressure of Ar gas must be placed in the container
to double the equilibrium water vapor pressure to 0.0656 atm?

A 1 liter solution of diluted liquid chloroform with toluene is
in a sealed container. The mole fraction of chloroform in the gas
phase was measured at 1500 ppmv once the solution was prepared. The
molecular weight is 119.35 g/mol for chloroform and 92.13 g/mol for
toluene. The vapor pressure of chloroform and toluene are 151 mmHg
and 28.1 mmHg, respectively.
What must the volume of liquid chloroform be in order to
make a 1.0 liter total volume solution?
What...

The vaporization of 1 mole of liquid water (the system) at 100.9
degrees C, 1.00 atm, is endothermic.
H2O(l) + 40.7kJ ---> H2O (g)
Assume at exactly 100.0 degrees C and 1.00 atm total pressure,
1.00 mole of liquid water and 1.00 mole of water vapor occupy 18.80
mL and 30.62 L, respectively.
1. Calculate the work done on or by the system when 3.65 mol of
liquid H2O vaporizes. Answer in J
2. Calculate the water's change in internal...

8.33 kg of steam at temperature of 150 ∘C has 2.23×107 J of heat
removed from it. Determine the final temperature and phase of the
result once the heat has been removed if the heat is removed at
constant pressure during the gas phase. For this problem, use the
specific heat (at constant pressure) for water as 1850 J/kg∘C , the
latent heat of vaporization as 2.256×106 J/kg , the specific heat
of liquid water as 4186 J/kg∘C , the...

Let's say you completely boil 3.96 kg of rubbing alcohol at
constant air pressure 99.7 kPa. What will be the resulting volume
of vapor, in m3, assuming it behaves like an ideal gas? (Possibly
useful: density of rubbing alcohol: 0.786 kg/liter, molar mass of
rubbing alcohol: 60.1 kg/kmol, gas constant R = 8.314 kJ K−1
kmol−1. Beware K vs °C, Pa vs kPa, g vs kg, mol vs kmol, etc.)

At 0,00℃, for H2O (l) the saturation pressure P = 4,581 dry (i.e., the water vapor equilibrium pressure)
and the vaporization heat, ?vapHm = 45,067 kJ mol-1. The steam can be regarded as an ideal gas.
a) Calculate water pressure at 100,00?C with the assumption that ?vapHm is a constant between
0,00 and 100,00℃.
b) Between 0,00 and 100,00℃, ?Cp,m for water evaporation can be adapted to the expression
?Cp,m = (-51,22 + 0,03153T) J K-1 mol-1.
Derive an expression between 0,00 and 100,00?C for ?vapHm as a function of T as well as
calculate P at 100?C.

A cylinder of indefinite height contains a frictionless and
massless piston. The
part of the cylinder above the piston is exposed to the
atmosphere with P=1.000 atm.
In the bottom of the cylinder are 5.000 kmoles of a liquid that
has a boiling point
equal to 320.0 K at P=1.000 atm., a heat of vaporization of
2.520 X 107J/kmole, and
cp = a+bT-1 for the liquid phase, where a=3.000x104
J/kmole/K and b=2.500x104J/kmole.
A. At constant pressure, how much heat is required...

Quantity
per gram
per mole
Enthalpy of fusion
333.6 J/g
6010. J/mol
Enthalpy of vaporization
2257 J/g
40660 J/mol
Specific heat of solid
H2O (ice)
2.087 J/(g·°C) *
37.60 J/(mol·°C) *
Specific heat of liquid
H2O (water)
4.184 J/(g·°C) *
75.37 J/(mol·°C) *
Specific heat of gaseous
H2O (steam)
2.000 J/(g·°C) *
36.03 J/(mol·°C) *
At 1 atm, how much energy is required to heat 49.0 g of H2O(s)
at − 18.0 °C to H2O(g) at 135.0 °C? Heat transfer...

A cylinder of volume 0.320 m3 contains 11.1 mol of
neon gas at 19.1°C. Assume neon behaves as an ideal gas.
(a) What is the pressure of the gas?
Pa
(b) Find the internal energy of the gas.
J
(c) Suppose the gas expands at constant pressure to a volume of
1.000 m3. How much work is done on the gas?
J
(d) What is the temperature of the gas at the new volume?
K
(e) Find the internal energy...

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