Question

A calorimeter contains 75.0 g of water at an initial temperature of 25.2 °C. 151.28 g of copper metal at a temperature of 95.5 °C was placed in the calorimeter. The equilibrium temperature was 36.2 °C. The molar heat capacity of water is 75.4 J / mol °C. Determine the molar heat capacity of the copper.

Answer #1

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....

An 100-g aluminum calorimeter contains 280 g of water at an
equilibrium temperature of 20°C. A 170-g piece of metal, initially
at 277°C, is added to the calorimeter. The final temperature at
equilibrium is 32°C. Assume there is no external heat exchange. The
specific heats of aluminum and water are 910 J/kg·K and 4190
J/kg·K, respectively. The specific heat of the metal is closest
to:
a) 270 J/kg·K.
b) 240 J/kg·K.
c) 330 J/kg·K.
d) 390 J/kg·K.
e) 360 J/kg·K.

An iron calorimeter of mass 153 g contains 260 g of water. The
system is in thermal equilibrium at +10°C. We place two blocks of
metal in the water: one is a 45 g piece of copper with an initial
temperature of +61°C; the second piece has a mass of 75 g and is
initially at +100°C. The combined system reaches a final
equilibrium temperature of +41°C. Calculate the specific heat
capacity of the unknown second piece of metal.

1. A calorimeter contains
125g of water at 40.6*C. A 7.55 g object is 63.0C is inside the
calorimeter. When equilibrium is reached, the new temperature of
water and the metal object is 42.6*C, determine the specific heat
of the metal object.
2. If the equivalence point
was determined to be 7.6 for an acid base titration of acetic acid
and sodium hydroxide, calculate the molarity of the acetic acid in
the hot sauce if 6.00mL of 0.1 M NAOH...

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°

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...

A 100 g aluminum calorimeter contains 250 g of water. The two
substances are in thermal equilibrium at 10°C. Two metallic blocks
are placed in the water. One is a 50 g piece of copper at 82°C. The
other sample has a mass of 78 g and is originally at a temperature
of 100°C. The entire system stabilizes at a final temperature of
20°C. Determine the specific heat of the unknown second sample.

A calorimeter contains 33.0 mL of water at 15.0 ∘C . When 2.10 g
of X (a substance with a molar mass of 46.0 g/mol ) is added, it
dissolves via the reaction
X(s)+H2O(l)→X(aq)
and the temperature of the solution increases to 28.0 ∘C .
Calculate the enthalpy change, ΔH, for this reaction
per mole of X.
Assume that the specific heat of the resulting solution is equal
to that of water [4.18 J/(g⋅∘C)], that density of water is 1.00...

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 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).

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