Question

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?

Answer #1

Water's heat of fusion is 80. cal/g, and its specific heat is
1.0 cal/g.celsius. Some velomobile seats have been designed to hold
ice packs inside their cushions. If you started a ride with ice
packs that held 1200 of frozen water at 0 celsius , and the
temperature of the water at the end of the ride was 32 celsius ,
how many calories of heat energy were absorbed?

Suppose the latent heat of vaporization of water is 540 cal/g.
how much heat (in calories) must be added to 50 grams of water at
an initial temperature of 20 C ( C represent degree Celsius) to a.
heat it to the boiling point?
b. then completely convert the water to steam?

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...

What mass of steam at 160 degree C must be mixed with 150g of ice
at 0 degree C, in a thermally insulated container, to produce
liquid water at 60 degrees C? Specific heat (heat capacity) of
water is 1 cal/gC, of steam 0.48 cal/gC and of ice 0.5 cal/gC.
Latent heat of melting for ice is 80 cal/g. Latent heat of
vaporization for steam is 540 cal/g.

The heat of fusion of water is 79.9 cal/g, the heat of
vaporization of water is 540 cal/g, and the specific heat of water
is 1.00 cal/deg/g. How many grams of ice at 0 ° could be converted
to steam at 100 °C by 9,076 cal of heat?

803 cal of heat is added to 5.00 g ice at –20.0 °C.
What is the final temperature of the water?
SPecific heat H2O(s)= 2.087 J/(g*C)
Specific heat H2O(l)=4.184 J/(g*C)
Heat of fusion= 333.6 J/g

2. Sixty grams of water is at an initial temperature of 24
°C.
Calculate the heat required to completely convert the 100 ºC
water to steam. (The latent heat of vaporization of water is 540
cal/g.)
The heat required to completely convert the 100 ºC water to
steam is... kcal?
3. How much heat is required to raise the temperature of 140 g
of water from 12°C to 88°C? The specific heat capacity of water is
1 cal/g·°C.
The heat...

A 40-g block of ice is cooled to
−72°C
and is then added to 590 g of water in an 80-g copper
calorimeter at a temperature of 26°C. Determine the final
temperature of the system consisting of the ice, water, and
calorimeter. (If not all the ice melts, determine how much ice is
left.) Remember that the ice must first warm to 0°C, melt, and then
continue warming as water. (The specific heat of ice is 0.500 cal/g
· °C...

A 100g ice cube at 0°C is placed in 400g of water at 30°C. If
the container is perfectly insulated, what will be the final
temperature when all the ice has been melted? The specific heat of
water is 4.184 kJ/kg. K. The latent heat of fusion for water at 0°C
is approximately 334 kJ/kg (or 80 cal/g).

To change 25 kg of ice -10°C to steam 100°C, how much heat is
required? The specific heat of water is 4.184 kJ/kg. K. The latent
heat of fusion for water at 0°C is approximately 334 kJ/kg (or 80
cal/g), and the latent heat of vaporization at 100°C is about 2,230
kJ/kg (533 cal/g).

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