Question

The temperature of a 0.555 kg block of ice is lowered to -120°C. Heat (0.5159 MJ) is then transferred to the block of ice (assume ice is otherwise thermally isolated). What is the final temperature of the water in °C?

Answer #1

Question 1 : The temperature of a 0.555 kg block of ice is
lowered to -120°C. Heat (0.5159 MJ) is then transferred to the
block of ice (assume ice is otherwise thermally isolated). What is
the final temperature of the water in °C?
Question 2 : Calculate the time needed (seconds) to that up 285
mL of tomato soup from 4.0°C to 57°C in a 1100. watt microwave
oven. Assume that the density of tomato soup is 1.25 g/mL and...

A 10.84 kg block of ice has a temperature of -22.5o C. The
pressure is one atmosphere. The block absorbs 5.113×106 J of heat.
What is the final temperature of the liquid water? (Give your
answer in oC, but enter only the numerical portion--oC is
implied)
Tries 0/10

1. A 36.6-kg block of ice at 0 °C is sliding on a horizontal
surface. The initial speed of the ice is 9.02 m/s and the final
speed is 3.89 m/s. Assume that the part of the block that melts has
a very small mass and that all the heat generated by kinetic
friction goes into the block of ice, and determine the mass of ice
that melts into water at 0 °C.
2. A rock of mass 0.396 kg...

A 2.5 kg metallic block with an initial temperature of 80°C is
placed in a styrofoam cup containing 0.1 kg of ice at -15°C.
Assuming that no heat escapes from the cup what is the final
temperature of the metallic block? The specific heat of the metal
is 480 J/kg ∙ K, specific heat of ice is 2090 J/kg ∙ K, the latent
heat of fusion of water is 3.33 × 105 J/kg, and the specific heat
of water is...

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...

Suppose that 0.1 kg of ice at an initial temperature of -10°C are
put into 0.40 kg of water at an initial temperature of 20°C. Assume
the final temperature is 0°C. How many grams of ice will melt?
Specific heat capacity of water is 4,200 J/kg/°C. Specific heat of
fusion of water is 336,000 J/kg and specific heat capacity of ice
is 2,100 J/kg/°C.

A 41.9-kg block of ice at 0 °C is sliding on a horizontal
surface. The initial speed of the ice is 8.83 m/s and the final
speed is 3.69 m/s. Assume that the part of the block that melts has
a very small mass and that all the heat generated by kinetic
friction goes into the block of ice, and determine the mass of ice
that melts into water at 0 °C.

A 48.5-kg block of ice at 0 °C is sliding on a horizontal
surface. The initial speed of the ice is 8.24 m/s and the final
speed is 4.08 m/s. Assume that the part of the block that melts has
a very small mass and that all the heat generated by kinetic
friction goes into the block of ice, and determine the mass of ice
that melts into water at 0 °C.

2.50 kg of water at 90 (degrees of C) is contained in a
thermally-isolated container. A 1.50 kg chunk of ice at - 10
degrees C is added to the water, in the same thermally isolated
container. a.) Describe the final state of the system when it has
reached thermal equilibrium, give the final temperature and the
amount of ice let (if any). b.) Find the net change in entropy of
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A 24 g block of ice is cooled to −63◦C. It is added
to 572 g of water in a 98 g copper calorimeter at a temperature of
30◦C.
Find the final temperature. The specific heat of copper is 387
J/kg ·◦C and of ice is 2090 J/kg ·◦C. The
latent heat of fusion of water is 3.33 × 105 J/kg and its specific
heat is 4186 J/kg·◦C.
Answer in units of ◦C.

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