Question

What is the total heat flow if 28 grams of water at 12°C is cooled to become ice at –19°C? The specific heat of liquid water is 4.18 J/g • °C; the specific heat of ice is 2.1 J/g • °C. The heat of fusion of ice is 333 J/g, and the freezing point of water is 0.0°C.

Answer #1

Energy required to remove energy from 12°C to 0°C

Q1 = mass * specific heat * ∆T

= 28*4.18*(12-0)

= 1404.48 joules

Energy removed to change the phase

Q2 = mass * ∆H(fus)

= 28*333

= 9324 joules

Energy remived to change 0°C to -19°C

Q3 = mass * specific heat of ice * ∆T

= 28*2.1*(0-(-19)

= 1117.2 joules

Total heat = Q1 + Q2 + Q3

= 1404.48 + 9324 + 1117.2

= 11845.68 joules

If you have any query please comment

If you satisfied with the solution please like it thankxx

A quantity of ice at 0.0 °C was added to 33.6 g of water at 41.0
°C to give water at 0.0 °C. How much ice was added? The heat of
fusion of water is 6.01 kJ/mol, and the specific heat is 4.18
J/(g•°C). ______ grams

100. g of ice at 0 degrees C is added to 300.0 g of water at 60
degrees C. Assuming no transfer of heat to the surroundings, what
is the temperature of the liquid water after all the ice has melted
and equilibrium is reached?
Specific Heat (ice)= 2.10 J/g C
Specific Heat (water)= 4.18 J/g C
Heat of fusion = 333 J/g
Heat of vaporization= 2258 J/g

Calculate the energy needed to heat 14.6 g ice
at -10.0 °C to liquid water at
70.0 °C. The heat of vaporization of water = 2257
J/g, the heat of fusion of water = 334 J/g, the specific heat
capacity of water = 4.18 J/g·°C, and the specific heat capacity of
ice = 2.06 J/g·°C.

How many grams of ice at -14°C must be added to 710 grams of
water that is initially at a temperature of 81°C to produce water
at a final temperature of 12°C. Assume that no heat is lost to the
surroundings and that the container has negligible mass. The
specific heat of liquid water is 4190 J/kg·C° and of ice is 2050
J/kg·C°. For water the normal melting point is 0.00°C and the heat
of fusion is 334 × 103...

Calculate the amount of heat required to change 35.0g ice at
-25.0 C to steam at 125 C (Heat of fusion = 333 J/g; heat of
vaporization = 2260 J/g; Specific heats: ice = 2.09 J/g*K, water =
4.18 J/g*K, steam = 1.84 J/g*K)

The heat of combustion of bituminous coal is 2.50 × 10 4 J/g.
What quantity of the coal is required to produce the energy to
convert 27.0 kg of ice at 0.00°C to steam at 100.°C? specific heat
(ice) = 2.10 J/g°C specific heat (water) = 4.18 J/g°C heat of
fusion = 333 J/g heat of vaporization = 2258 J/g

How many grams of ice at -13°C must be added to 714 grams of
water that is initially at a temperature of 83°C to produce water
at a final temperature of 11°C. Assume that no heat is lost to the
surroundings and that the container has negligible mass. The
specific heat of liquid water is 4190 J/kg·C° and of ice is 2050
J/kg·C°. For water the normal melting point is 0.00°C and the heat
of fusion is 334 × 103...

4. Steam is condensed at 100oC to water which is
cooled to 0oC and frozen to ice. What are the molar
enthalpy and entropy changes for this process? Assume that the
average specific heat of water is 4.2JK-1 g-1
and the enthalpy of vaporization at the boiling point and the
enthalpy of fusion at the freezing point are 2258.1 and 333.5 J
g-1 respectively.
(Note: Convert Jg-1 to J mol-1)

An 11 g ice cube at -12˚C is put into a Thermos flask containing
145 cm3 of water at 24˚C. By how much has the entropy of
the cube-water system changed when a final equilibrium state is
reached? The specific heat of ice is 2200 J/kg K and that of liquid
water is 4187 J/kg K. The heat of fusion of water is 333 ×
103 J/kg.
and
A 6.0 g ice cube at -21˚C is put into a Thermos...

A 0.4-L glass of water at 20°C is to be cooled with ice to 5°C.
The density of water is 1 kg/L, and the specific heat of water at
room temperature is c = 4.18 kJ/kg·°C. The specific heat
of ice at about 0°C is c = 2.11 kJ/kg·°C. The melting
temperature and the heat of fusion of ice at 1 atm are 0°C and
333.7 kJ/kg.
A) Determine how much ice needs to be added to the water, in...

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 34 minutes ago

asked 39 minutes ago

asked 44 minutes ago

asked 48 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 2 hours ago

asked 3 hours ago

asked 3 hours ago

asked 3 hours ago

asked 3 hours ago