Question

A calorimeter contains 82.4 grams of water at 20.9 °C. A 156 -gram piece of an unknown metal is heated to 81.9 °C and dropped into the water. The entire system eventually reaches 26.6 °C. Assuming all of the energy gained by the water comes from the cooling of the metal—no energy loss to the calorimeter or the surroundings—calculate the specific heat of the metal. The specific heat of water is 4.18 J/g · °C _____J/g · °C

Answer #1

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 72.5 gram piece of magnesium is heated to a temperature of
98.90ºC. The metal is then dropped into 40.0 grams of water at a
temperature of 18.50ºC inside a perfect calorimeter. Calculate the
final temperature of the water in the calorimeter. The specific
heat capacity for magnesium is Cp = 1.020 J/g·ºC.
Tfinal = ºC

There is 300 grams of water in the 200-gram calorimeter cup
(inner can). Both are at room temperature of 20 degrees Celsius. A
100-gram metal sample with an initial temperature of 90 degrees
Celsius is placed in the calorimeter resulting. The resulting final
temperature of the system is 30 degrees Celsius. If the calorimeter
can has a specific heat of 0.2 cal/g-C degree, determine the
specific heat of the metal sample

A coffee-cup calorimeter contains 130.0 g of water at 25.3 ∘C .
A 124.0-g block of copper metal is heated to 100.4 ∘C by putting it
in a beaker of boiling water. The specific heat of Cu(s) is 0.385
J/g⋅K . The Cu is added to the calorimeter, and after a time the
contents of the cup reach a constant temperature of 30.3 ∘C .
Part A
Determine the amount of heat, in J , lost by the copper block....

1. A 78.0 g piece of metal at 89.0°C is placed in 125 g of water
at 21.0°C contained in a calorimeter. The metal and water come to
the same temperature at 27.0°C.
- How much heat (in J) did the metal give up to the water?
(Assume the specific heat of water is 4.18 J/g·°C across the
temperature range.)
- What is the specific heat (in J/g·°C) of the metal?
2. A 0.529 g sample of KCl is added...

1. A 74.2-g piece of metal is heated to 89.55 degrees C and
dropped into 52.0 g of water at 23.22 degrees C in a calorimeter
with the heat capacity of 41.0 J/C . The
final temperature of the system is 27.60 degrees C.
a) Assuming that the metal does not react with water and
Cs(H2O) = 4.18 J/g*C , calculate
the specific heat capacity of the metal in
J/g*C
b) Most metals have the same molar heat capacity of...

1a) A 25.5-g piece of lead initially at 98.6 °C is submerged
into 122.3 g of water at 20.9 °C. What is the final temperature of
the metal once the metal and water reaches thermal equilibrium? The
specific heats of lead and water are 0.128 J/g·°C and 4.18 J/g·°C,
respectively.

A 10.67-gram -23.0°C piece of ice drops into a calorimeter
containing 150.00-gram 93.7 °C of the water. What is the final
temperature? (Swater = 4.184 J/g° C, Sice = 2.082 J/g° C, Heat of
fusion= 334.7 J/g)

A piece of titanium metal with a mass of 20.8 g is heated in
boiling water to 99.5 0C and then dropped into a coffee
cup calorimeter containing 75.0 g of water at 21.7
0C.When thermal equilibum is reached, the final
temperature is 14.30C.Calculate the specific heat
capacity of titanium. ( Specific Heat Capacity of H2O
(l) =4.184 J g-1 0C-1)

A calorimeter made of copper (c=0.0923 cal/g-C°) of mass 300 g
contains 450 grams of water. The container is initially at room
temperature, 20°C. A 1 kg block of metal is heated to 100°C and
placed in the water in the calorimeter. The final temperature of
the system is 40°C. What is the specific heat of the metal?
A.
0.159 kcal/kg-C °
B.
0.591 kcal/kg-C°
C.
0.519 kcal/kg-C°
D.
0.915 kcal/kg-C°

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