Question

A 180 g copper bowl contains 150 g of water, both at 19.0°C. A very hot 490 g copper cylinder is dropped into the water, causing the water to boil, with 10.5 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 of water is 1 cal/g·K, and of copper is 0.0923 cal/g·K. The latent heat of vaporization of water is 539 Cal/kg.

Answer #1

A 190 g copper bowl contains 110 g of water, both at 20.0°C. A
very hot 430 g copper cylinder is dropped into the water, causing
the water to boil, with 2.42 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...

A 190 g copper bowl contains 230 g of water, both at 22.0°C. A
very hot 430 g copper cylinder is dropped into the water, causing
the water to boil, with 6.44 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...

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...

A 160 g copper bowl contains 170 g of water, both at 22.0°C. A
very hot 390 g copper cylinder is dropped into the water, causing
the water to boil, with 14.9 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...

A 170 g copper bowl contains 245 g of water, both at 20.0°C. A
very hot 300 g copper cylinder is dropped into the water, causing
the water to boil, with 5.45 g being converted to steam. The final
temperature of the system is 100°C. Neglect energy transfers with
the environment.
(c) What is the original temperature of the cylinder? (in
celcius)

A 100 g copper bowl contains 500 g of water, both at 20◦C. A
very hot 300 g copper cylinder is dropped into the water, causing
the water to boil, with 5 g of the water being converted to steam,
and the final temperature of the system is 100◦C. What is the
original temperature of the cylinder?

A well-insulated 0.2kg copper bowl contains 0.10kg of ice, both
at −10◦ C. A very hot 0.35kg copper cylinder is dropped into it and
the lid quickly closed. The final temperature of the system is
100◦C, with 5g of steam in the container.
(a) How much heat was transferred to the water (in all
phases);
(b) How much to the bowl?
(c) What must have been the original temperature of the
cylinder?
The specific heat of copper is 386 J/kg·K....

An iron boiler of mass 180 kg contains 770 kg of water at 21 ∘C.
A heater supplies energy at the rate of 58,000 kJ/h. The specific
heat of iron is 450 J/kg⋅C∘, the specific heat of water is 4186
J/kg⋅C∘, the heat of vaporization of water is 2260 kJ/kg⋅C∘. Assume
that before the water reaches the boiling point, all the heat
energy goes into raising the temperature of the iron or the steam,
and none goes to the vaporization...

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
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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?

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