Question

A 60 kg block of ice begins at -60 degrees the specific heat of ice is 2090 j/(kg)C. The latent heat of fusion of water is 3.3 x 10^5 and the latent heat of vaporization is 2.3 x 10^6 J/kg. How much energy is required to heat the ice to 0 degrees Celcius (melting point)?

How much energy is required to heat the ice from -50C to the melting point and melt the ice?

How much energy is required to heat the ice from -50C to the melting point, melt the ice, and raise the temperature of the water to 100C?

How much energy is required to heat the ice from -50C to the melting point, melt the ice, and raise the temperature of the water to 100C, then evaporate the water?

Answer #1

suppose the specific heat of ice and water is 0.49 cal/g. C ( C
represent degree Celsius) and 1.0 cal/g. C. the latent heat of
fusion of water is 80 cal/g. how much heat (in calories) is
required for 100 grams of ice with an initial temperature of -10 C
to a. raise the ice's temperature to the melting point? b. then
completely melt the ice to water? c. finally, raise the water's
temperature to 50 C?

How much energy is required to change a 23 g ice cube from ice
at − 12 ◦ C to steam at 101 ◦ C? The specific heat of ice is 2090 J
/ kg · ◦ C and of water 4186 J / kg · ◦ C. The latent heat of
fusion of water is 3 . 33 × 10^5 J / kg, its latent heat of
vaporization is 2 . 26 × 10^6 J / kg, and the...

The specific heat of water in its solid phase (ice) is 2090
J/(kg K), while in the liquid phase (water) its specific heat is
4190 J/(kg K). Water's latent heat of fusion is 333,000 J/kg.
If you have a 2kg block of ice at -90 degrees C and you add
1,000,000 J of heat, what is its new temperature?

You have a pitcher with 2.00 L of water at an initial
temperature of 12.0 oC and you wish to add ice to it to bring the
temperature down. If the ice starts at an initial temperature of T1
= -18.4 oC, calculate the mass of ice required to reach a final
state of all liquid water at 0.00 oC. *****Assume no heat is gained
or lost to the surroundings.*****
More information:
Melting point of water - 0.00 degrees celcius...

How much heat must be removed to make ice at -10 degrees C from
2kg of water at 20 degrees C (The latent heat of fusion for water
is.25X10^5 J/kg. The specific heat of water is 4190 J/kg K and for
ice is 2090 J/kg K.)
a. 7.95 X10^5
b. 8.37 X10^5
c.8.75 X10^5
d. 2.09x10^5

You have a block of ice at 32 degrees F, and a block of copper
at some other temperature. The blocks have equal mass. Exactly the
same amount of heat is added to each block. This causes the ice to
melt completely, but not to warm up past 32 degrees F. The copper
stays well below its melting point.
How much does the copper expand?
(Express your answer as a percentage, e.g. "the length of the
copper increases by 1%.")...

What is the final equilbrium temperature when 40.0 grams of ice
at -12.0 degrees C is mixed with 20.0 grams of water at 32 degrees
C? The specific heat of ice is 2.10 kJ/kg degrees C, the heat of
fusion for ice at 0 degrees C is 333.7 kJ/kg, the specific heat of
water 4.186 kJ.kg degrees C, and the heat of vaporization of water
at 100 degrees C is 2,256 kJ/kg.
A. How much energy will it take to...

How much energy is required to change a 34 g ice cube from ice
at −10◦C to steam at 119◦C? The specific heat of ice is 2090 J/kg ·
◦ C, the specific heat of water is 4186 J/kg · ◦ C, the specific
heat of stream is 2010 J/kg · ◦ C, the heat of fusion is 3.33 × 105
J/kg, and the heat of vaporization is 2.26 × 106 J/kg. Answer in
units of J

How much heat is required to change m=1kg of ice at
-6°C into water at 60°C? cw= 4190
J/kg*K (specific heat of water), Lf= 333 kJ/kg (latent
heat of fusion of ice), cice= 2100 J/kg*K

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...

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