How much energy in kJ is required to fully vaporize (at
temperature of boiling point = 2525C) a 270g sample of Al(s),
initially at 25C?
(Enthalpy of vap = 300. kJ/mol, enthalpy of fusion = 11.
kJ/mol)
(specific heat of aluminum for both solid and liquid form = 0.9
J/(K * g))
(temperature of melting point = 625C, temp of boiling point =
2525C)
At 1 atm, how much energy in kJ is required to heat 85.0 g H 2 O
( s ) at − 10.0 ∘ C to H 2 O ( g ) at 167.0 ∘ C? Use the heat
transfer constants found in this table.
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...
A piston–cylinder device initially contains 2 kg water in 1 m3
at 500 kPa. The system then cools down and the volume drops to half
and pressure of 300 kPa. At this state, the piston is resting on a
set of stops, and the mass of the piston is such that a pressure of
500 kPa is required to move it. (a) Show the process on a P-v, T-v
and P-T diagrams with respect to saturation lines and determine,
(b)...
How much energy (in kJ) is required to convert a 2.56 lb block
of ice at -12.5oF to steam at 234oF? Use the space provided on this
page to draw a complete heating curve, labeling the axes and each
important point on the graph. Below the graph, show your
calculations and the final answer.
How much heat is required to melt 1 kg of solid water at 0
°C?
How much heat is released when freezing 1 kg of solid water at 0
°C?
How much heat is released when freezing 1 kg of supercooled
water at -10 °C?
How much heat is required to boil 1 kg of superheated water at
110 °C?
How much heat is required to convert 1 kg of ice at -20 °C to
water vapor at 120 °C?...
Determine
how much
energy in kJ would be transferred if 300.0 grams
of steam (gaseous
water) at 150.0
̊C
is cooled to ice
(solid water)
at -20.0
̊C.
The specific
heat
of steam is
1.86
J/(g∙ ̊C),
the
specific heat
of ice is 2.06
J/(g∙ ̊C),
the heat of fusion of water
is 333
J/g, and
the heat
of vaporization is 2256 J/g.
1)Consider water at 500 kPa and a specific volume of 0.2
m3/kgm3/kg. What is the temperature (in °C)?
2)Consider water at 500 kPa and a specific volume of 0.2
m3/kgm3/kg. What is the quality (on a 0 to 1 scale)?
3)Consider water at 1400 kPa and 200°C. What is the specific
volume (in m3/kgm3/kg)?
5. How many kJ of energy are required to change 1.00 m^3 of pure
water by 1.0*C? Assume a perfect system. The specific heat of the
water is 4.184 J/g*C. The density of water is 1.000 g/mL.
6. 2.500 grams of metal X (molar mass 65.39 g/mole) was reacted
with 100.0 mL of a 1.500 M HCl solution in a coffee cup
calorimeter. The temperature went from 12.50 *C to 40.50 *C.
Determine the reaction enthalpy per mole of metal...