Question

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 to 62.2 g of water in a calorimeter. If the temperature decreases by 1.16°C, what is the approximate amount of heat (in J) involved in the dissolution of the KCl, assuming the heat capacity of the resulting solution is 4.18 J/g°C? Is the reaction endothermic or exothermic?

Answer #1

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?

A 0.505 g sample of KCl is added to 61.0 g of water in a
calorimeter. If the temperature decreases by 1.06°C, what is the
approximate amount of heat (in J) involved in the dissolution of
the KCl, assuming the heat capacity of the resulting solution is
4.18 J/g°C?

A 53.0-g metal weight, heated to 87.50°C, is placed into 191 g
of water at 21.05°C contained in a perfectly insulating thermos
flask. After some time, the temperature inside the thermos flask
stabilizes at 23.80°C.
The specific heat capacity of water is approximately 4.18
J/K/g in the temperature range 16°C - 61°C.
Calculate the specific heat capacity of the metal.

A metal sample weighing 72.1 g is placed in a hot water bath at
95.0 oC. The calorimeter contains 42.3 g of deoinized water. The
initial temperature of the water is 22.3 oC. The metal is
transferred to the calorimeter and the final temperature reached by
the water + metal is 32.2 oC.
A. Calculate ∆T for the water (Tfinal – Tinitial).
B. Calculate ∆T for the metal.
C. The specific heat of water is 4.18 J/goC. Calculate the
specific...

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...

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).

A 2.00 g sample of KCl is added to 35.0 g H2O in a styrofoam cup
and stirred until dissolved. The temperature of the solution drops
from 24.8 to 21.6 ˚C. Assume that the specific heat and density of
the resulting solution are equal to those of water, 4.18 J/(g ˚C)
and 1.00 g/mL, respectively and assume that no heat is lost to the
calorimeter itself, nor to the surroundings. KCl(s) + H2O(l) -->
KCl(aq) ∆H = ? a) Is...

In an experiment, 22.5 g of metal was heated to 98.0°C and then
quickly transferred to 150.0 g of water in a calorimeter. The
initial temperature of the water was 27.0°C, and the final
temperature after the addition of the metal was 32.5°C. Assume the
calorimeter behaves ideally and does not absorb or release
heat.
What is the value of the specific heat capacity (in J/g•°C) of
the metal?

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

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 3 minutes ago

asked 12 minutes ago

asked 44 minutes ago

asked 44 minutes ago

asked 44 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 2 hours ago

asked 2 hours ago

asked 2 hours ago

asked 2 hours ago