Question

Answer the following questions:

a) A calorimeter, specific heat capacity 500.0 J/kgC, mass 200.0 g, contains 300.0 g of water at 40.0 C. If 50.0 g of ice at 0.00 C is dropped into the water and stirred, the temperature of the mixture when the ice has melted is 23.8 C. Calculate the heat of fusion of ice.

b) What is the final temperature attained when 900.0 g of ice at 0.00 C is dropped into 3400.0 g of water at 93.3 C in a calorimeter having a mass of 1350 g of water at 93.3 C in a calorimeter having a mass of 1350 g and a specific heat of 400.0 J/kgC

Answer #1

A 6.40 g sample of iron (specific heat capacity = 0.451 J/g*C)
is placed in a boiling water bath until the temperature of the
metal is 100.0*C. The metal is quickly transferred to 119.0g of
water at 25.0*C in a calorimeter (specific heat capacity of water =
4.18 J/g*C). Determine the final temperature of the water in the
calorimeter (3 significant figures).

300.0 g of copper is heated to 100.0*C and transferred quickly
to a calorimeter containing 400.0 grams of water initially at
25.0*C. If the final temperature is 29.4*C, calculate the specific
heat of copper. The specific heat of water is 4.18 J/g-*C. What
assumptions must be made about the calorimeter? How is the first
law of thermodynamics and law of conservation of energy used in
this experiment.

A 6.40 g sample of iron (specific heat capacity =0.451 J/g*C) is
placed in a boiling water bath until the temperature of the metal
is 100.0*C. The metal is quickly transferred to 119.0g of water at
25.0*C in a calorimeter (specific heat capacity of water = 4.18
J/g*C). Determine the final temperature of the water in the
calorimeter (3 significant figures).

a 25.0g piece of aluminum (molar heat capacity of 24.03 J/g
degrees Celsius) is heated to 82.4 degrees Celsius and dropped into
a calorimeter containing water (specific heat capacity of water is
4.18 J/g degrees Celsius) initially at 22.3 degrees Celsius. The
final temperature of the water is 24.98 degrees Celsius. Calculate
the mass of water in the calorimeter.

A 500.0-g sample of an element at 153°C is dropped into an
ice-water mixture; 109.5-g of ice melts and an ice-water mixture
remains. Calculate the specific heat of the element from the
following data:
Specific heat capacity of ice: 2.03 J/g-°C
Specific heat capacity of water: 4.18 J/g-°C
H2O (s) → H2O (l), ΔHfusion: 6.02 kJ/mol (at 0°C)
a) If the molar heat capacity of the metal is 26.31 J/mol-°C,
what is the molar mass of the metal, and what...

An insulated aluminum calorimeter vessel of 150 g mass contains
300 g of liquid nitrogen boiling at 77 K. A metal block at an
initial temperature of 303 K is dropped into the liquid nitrogen.
It boils away 15.8 g of nitrogen in reaching thermal equilibrium.
The block is then withdrawn from the nitrogen and quickly
transferred to a second insulated copper calorimeter vessel of 200
g mass containing 500 g of water at 30.1 degrees celsius. The block
coolds...

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

A 40.0 g Ice Cube floats in 200.0 g of water in a 100.0 g copper
cup! All are at a temperature of 0.000C. Then, a piece of lead at
98.00C is dropped into the cup, and the final equilibrium
temperature is 12.00C. The specific heat of water and ice is 1.00
cal/g 0C, the specific heat of copper is 0.0924 cal/g 0C, the
specific heat of lead is 0.0305 cal/g 0C, and the heat of fusion of
ice is...

A calorimeter contains 500gm of water and 300gm of ice, all at a
temperature of 0 C. A block of metal of mass 1000gm is taken from a
furnace where its temperature was 240 C and is dropped quickly into
the calorimeter. As a result, all the ice is just melted. what
would the final temperature of the system have been if the mass of
the block had been twice as great? Neglect heat loss from the
calorimeter, and the...

Dissolving 3.00 g of CaCl2(s) in 200.0 g of water in a
calorimeter at 22.4 °C causes the temperature to rise to 25.8 °C.
What is the approximate amount of heat involved in the dissolution,
assuming the heat capacity of the resulting solution is 4.18 J/g
°C? Is the reaction exothermic or endothermic?

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