Question

describe what happens to the temperature of liquid water between 0 and 100 degrees celcius when heat energy is transferred to it at a constant rate

Answer #1

100 g of solid ice at 0 degree Celcius is added to 500 g of
liquid water at 90 degree celcius. What is the final temperature?
What initial water temperature is required so that 10 g of ice
remain once equilibrium has been reached?

What is the final equilbrium temperature when 40.0 grams of ice
at -12.0 degrees C is mixed with 20.0 grams of water at 32 degrees
C? The specific heat of ice is 2.10 kJ/kg degrees C, the heat of
fusion for ice at 0 degrees C is 333.7 kJ/kg, the specific heat of
water 4.186 kJ.kg degrees C, and the heat of vaporization of water
at 100 degrees C is 2,256 kJ/kg.
A. How much energy will it take to...

Calculate the heat flow when 18.7 g of water is heated from 25
degrees celcius to 68.2 degrees celcius (specific heat capacity for
water=4.184J/g.k

a 36.9g sample of metal is heated to 100.0 degrees celcius, and
then added to a calorimeter containing 141.5g of water at 23.1
degrees celcius. the temperature of the water rises to a maxiumum
of 25.2 degrees celcius before cooling back down.
a) did the water absorb heat or did it release heat?
b) how many joules of heat was exchanged between the water and
the metal?
c) what is the identity of the metal?

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 were analyzing an unknown that boiled at a temperature
above 100 degrees celcius, how could you modify the experiment so
that you COULD determine the boiling point of the unknown liquid?
explain

You
place 20g of ice initially at -10 degrees celcius and 200g of an
unknown substance initially at 90 degrees celcius together in an
insukated container. You find that the final temperature of the
system is 34.6 degrees celcius and note that the unknown substance
did not change phase. Given that the specific heat of ice is 2.04
kJ/kg•K, the specific heat of liquid water is 4.18 kJ/kg•K, and the
heat of fusion of water is 334 kJ/kg, find the...

How much work is needed to cool 0,500 litres of water from +10,0
degrees celcius to ice that has the temperature -20,0 degrees
celcius if the cooling machine that is being used is a carnot
process that works between +20 degrees celcius to -20 degrees
celcius?

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...

Some ice at -15 degrees celcius with a mass of 0.45 kg is
dropped into a highly insulated cup (no heat flows into or out of
cup) with 3.0 kg water that is at 20 degrees celcius.
Determine if all the ice has melted
What if the final temperature of the water in the cup?

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