Question

When 15.0 g of ice at 0°C is melted in 100 g of water at 20.0°C, the final temperature is 9.5°C. Find the heat of fusion of ice, based on this data.

Answer #1

Here we have given that,

Mass of ice = 15.0 g

Temp of ice = 0°C

Mass of water = 100 g

Temp of water = 20.0°C,

final temperature= 9.5°C.

Specific heat of water s = 4.187 J/g-C

To Find the heat of fusion of ice,

So that

On applying the formula

q = ms(deltaT)

q = 100 × 4.187 × (9.5 -20)

q = -4396.35 J

This represents the heat removed from the water, hence its negative sign.

By the laws of thermodynamics, this means that the ice cubes in the water absorbed +4396.35 J of heat.

So that, To find the heat of fusion of ice, f, according to f = q ÷ m by dividing the heat, q, absorbed by the ice.

f = q/m = 4396.35/15 = 293.09 J/g

Which is our required answer.

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

Steam at 100°C is added to ice at 0°C.
(a) Find the amount of ice melted and the final temperature when
the mass of steam is 14 g and the mass of ice is 65 g.
(b) Repeat with steam of mass 4.0 g and ice of mass 65
g.

Steam at 100°C is added to ice at 0°C.
(a) Find the amount of ice melted and the final temperature when
the mass of steam is 10.0 g and the mass of ice is 51.0 g.
g
°C
(b) Repeat this calculation, when the mass of steam as 1.00 g and
the mass of ice is 51.0 g.
g
°C

Steam at 100°C is added to ice at 0°C.
(a) Find the amount of ice melted and the final temperature when
the mass of steam is 14 g and the mass of ice is 46 g.
----g
----°C
(b) Repeat with steam of mass 2.9 g and ice of mass 46 g.
----g
-----°C

Steam at 100°C is added to ice at 0°C.
(a) Find the amount of ice melted (grams) and the final
temperature (celcius) when the mass of steam is 14 g and the mass
of ice is 51 g
(b) Repeat with steam of mass 2.8 g and ice of mass 51 g

Two 20.0-g ice cubes at –15.0 °C are placed into 225 g of water
at 25.0 °C. Assuming no energy is transferred to or from the
surroundings, calculate the final temperature of the water after
all the ice melts.

Two 20.0-g ice cubes at –15.0 °C are placed into 285 g of water
at 25.0 °C. Assuming no energy is transferred to or from the
surroundings, calculate the final temperature of the water after
all the ice melts.

Two 20.0-g ice cubes at –15.0 °C are placed into 265 g of water
at 25.0 °C. Assuming no energy is transferred to or from the
surroundings, calculate the final temperature, Tf, of the water
after all the ice melts.

A 100g ice cube at 0°C is placed in 400g of water at 30°C. If
the container is perfectly insulated, what will be the final
temperature when all the ice has been melted? 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).

Two 20.0-g ice cubes at –20.0 °C are placed into 285 g of water
at 25.0 °C. Assuming no energy is transferred to or from the
surroundings, calculate the final temperature, Tf, of the water
after all the ice melts. heat capacity of H2O(s) is 37.7 J/mol*K
heat capacity of H2O(l) is 75.3 J/mol*K enthalpy of fusion of H20
is 6.01 kJ/mol

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