Question

You want to cool 0.2 kg of coffee, initially at temperature Th =
80° C, with ice initially at Tc = 0° C. The specific heat of ice is
about 2108 J/kg K, and its latent heat of melting is about 334, 000
J/kg. You may take the specific heats of liquid water and coffee to
be the same: 4187 J/kg K.

A) Assume the coffee and ice form a closed system. You want them to
equilibrate at 40° C. How much ice should you add?

B) Suppose you add that ice, and find that after 20 minutes it
equilibrates with the coffee at 30° C rather than 40° C. How much
power does the coffee/ice system deliver to its surroundings, on
average

Answer #1

Please ask your doubts or queries in the comment section below.

Please kindly upvote if you are satisfied with the solution.

Thank you.

I place an ice cube with a mass of 0.223 kg and a temperature of
−35°C is placed into an insulated aluminum
container with a mass of 0.553 kg containing 0.452 kg of water. The
water and the container are initially in thermal equilibrium at a
temperature of 27°C. Assuming that no heat enters
or leaves the system, what will the final temperature of the system
be when it reaches equilibrium, and how much ice will be in the
container...

You initially have 2.0kg of ice in 3.0kg of water at 0°C. How
much total heat must be added in order to convert 2.0kg of the
entire sample to steam at 100°C? Separately determine the amount of
heat for each stage of this process.
Specific heat capacities (J/kg∙K) Latent heats (J/kg)
c ice = 2090 Lf = 33.5∙10^4
c water = 4186 Lv = 22.6∙10^5
c steam = 2010

You decide to put a 40.0 g ice cube at -10.0°C into a well
insulated coffee cup (of negligible heat capacity)
containing of water at 5.0°C. When equilibrium is
reached, how much of the ice will have melted? The specific heat of
ice is 2090 J/kg ∙ K, that of water is 4186 J/kg ∙ K, and the
latent heat of fusion of water is 33.5 × 104 J/kg.

At 0°C the latent heat of the ice<-->liquid transition is
3.34 × 105 J/kg. Clean water can be cooled a few degrees
below 0°C without freezing on an ordinary time-scale, even though
ice would have lower G. This non-equilibrium liquid state typically
remains until some disturbance (e.g. a bubble) triggers the
freezing.
1) What is the entropy difference between 4 kg of liquid water
and 4 kg of ice at 0°C?
2) The specific heat of liquid water is cpw=...

A 2.5 kg metallic block with an initial temperature of 80°C is
placed in a styrofoam cup containing 0.1 kg of ice at -15°C.
Assuming that no heat escapes from the cup what is the final
temperature of the metallic block? The specific heat of the metal
is 480 J/kg ∙ K, specific heat of ice is 2090 J/kg ∙ K, the latent
heat of fusion of water is 3.33 × 105 J/kg, and the specific heat
of water is...

Q3. A cube with side lengths of 2.91 cm is heated to a constant
temperature of 720 ◦C at the focal point inside of a parabolic
reflector. This has the effect of directing all of the cube’s
radiant energy toward a 3.92 kg pack of ice that is initially at
−19.0 ◦C. If the emissivity of the cube is 0.466, how long does it
take for the ice to completely vaporize? Use the following numbers
in your calculation:
• The...

You pour 200 g hot coffee at 78.7°C and some cold cream at
7.50°C to a 115-g cup that is initially at a temperature of 22.0°C.
The cup, coffee, and cream reach an equilibrium temperature of
62.0°C. The material of the cup has a specific heat of 0.2604
kcal/(kg · °C) and the specific heat of both the coffee and cream
is 1.00 kcal/(kg · C). If no heat is lost to the surroundings or
gained from the surroundings, how...

you pour 130 g hot coffee at 78.7°C and some cold cream at
7.50°C to a 115-g cup that is initially at a temperature of 22.0°C.
The cup, coffee, and cream reach an equilibrium temperature of
61.0°C. The material of the cup has a specific heat of 0.2604
kcal/(kg · °C) and the specific heat of both the coffee and cream
is 1.00 kcal/(kg · C). If no heat is lost to the surroundings or
gained from the surroundings, how...

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...

If you pour 0.600 kg of 20.0ºC water onto a 1.20-kg block of ice
(which is initially at 0 ºC), what is the final temperature? You
may assume that the water cools so rapidly that effects of the
surroundings are negligible. The specific heat of water is 4 186
J/(kg * ºC), the specific heat of ice is 2 090 J/(kg * ºC), and the
heat of fusion of water is 334 x103 J/kg.

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 17 minutes ago

asked 19 minutes ago

asked 41 minutes ago

asked 46 minutes ago

asked 55 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 2 hours ago

asked 2 hours ago

asked 2 hours ago

asked 2 hours ago