Question

How much heat must be added to 100 g of water at an initial
temperature of 50^{o}C to completely evaporate it? Specific
heat capacity of water is 1 cal/(^{o}C·g), and latent heat
of vaporization is 540 cal/g.

Answer #1

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...

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?

How much heat must be added to 417 g of water at an initial
temperature of 14°C to
(a) Heat it to the boiling point?
(b) completely convert the 100°C water to steam?

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?

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?

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).

A 110 g copper bowl contains 100 g of water, both at 22.0°C. A
very hot 360 g copper cylinder is dropped into the water, causing
the water to boil, with 7.52 g being converted to steam. The final
temperature of the system is 100°C. Neglect energy transfers with
the environment. (a) How much energy is transferred to the water as
heat? (b) How much to the bowl? (c) What is the original
temperature of the cylinder? The specific heat...

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.

Burns produced by steam at 100°C are much more severe than those
produced by the same mass of 100°C water. To verify this:
(a) Calculate the heat that must be removed from 6.00 g of 100°C
water to lower its temperature to 45.0°C.
kcal
(b) Calculate the heat that must be removed from 6.00 g of 100°C
steam to condense it and lower its temperature to 45.0°C.
kcal
(c) Calculate the mass of human flesh that the heat produced in...

How many joules heat must be added to 2.0 kg of ice at a
temperature of -30 °C to bring it to room temperature 20 °C?
(Specific heat capacity of ice is 2100 J/kg °C).
(Specific heat capacity of water is 4186 J/kg °C).
(Latent heat of water-ice is 3.33x105 J/kg)
Group of answer choices
126.52 kJ
959.44 kJ
4293.44 kJ
668.78 kJ

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