Question

How many grams of ice at -13°C must be added to 714 grams of
water that is initially at a temperature of 83°C to produce water
at a final temperature of 11°C. Assume that no heat is lost to the
surroundings and that the container has negligible mass. The
specific heat of liquid water is 4190 J/kg·C° and of ice is 2050
J/kg·C°. For water the normal melting point is 0.00°C and the heat
of fusion is 334 × 10^{3} J/kg. The normal boiling point is
100°C and the heat of vaporization is 2.26 × 10^{6}
J/kg

Answer #1

How many grams of ice at -14°C must be added to 710 grams of
water that is initially at a temperature of 81°C to produce water
at a final temperature of 12°C. Assume that no heat is lost to the
surroundings and that the container has negligible mass. The
specific heat of liquid water is 4190 J/kg·C° and of ice is 2050
J/kg·C°. For water the normal melting point is 0.00°C and the heat
of fusion is 334 × 103...

How many grams of ice
at -13°C must be added to 711 grams of water that is initially at a
temperature of 87°C to produce water at a final temperature of
10°C? Assume that no heat is lost to the surroundings and that the
container has negligible mass.
The specific heat of
liquid water is 4190 J/kg • C° and of ice is 2100 J/kg • C°. For
water the normal melting point is 0.00°C and the heat of fusion...

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 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

An insulated beaker with negligible mass contains a mass of
0.200 kg of water at a temperature of 81.7 ∘C.
How many kilograms of ice at a temperature of − 21.1 ∘C must be
dropped in the water to make the final temperature of the system
30.8 ∘C?
Take the specific heat for water to be 4190 J/(kg⋅K) , the
specific heat for ice to be 2100 J/(kg⋅K) , and the heat of fusion
for water to be 334 kJ/kg...

An insulated beaker with negligible mass contains a mass of
0.350 kg of water at a temperature of 69.4 ∘C.
How many kilograms of ice at a temperature of − 14.7 ∘C must be
dropped in the water to make the final temperature of the system
29.3 ∘C?
Take the specific heat for water to be 4190 J/(kg⋅K) , the
specific heat for ice to be 2100 J/(kg⋅K) , and the heat of fusion
for water to be 334 kJ/kg...

100. g of ice at 0 degrees C is added to 300.0 g of water at 60
degrees C. Assuming no transfer of heat to the surroundings, what
is the temperature of the liquid water after all the ice has melted
and equilibrium is reached?
Specific Heat (ice)= 2.10 J/g C
Specific Heat (water)= 4.18 J/g C
Heat of fusion = 333 J/g
Heat of vaporization= 2258 J/g

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.

Adding Ice to Water
An insulated beaker with negligible mass contains liquid water
with a mass of 0.340 kg and a temperature of 66.3 ∘C .
How much ice at a temperature of -17.9 ∘C must be dropped into
the water so that the final temperature of the system will be 22.0
∘C ?
Take the specific heat of liquid water to be 4190 J/kg⋅K , the
specific heat of ice to be 2100 J/kg⋅K , and the heat of...

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...

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