Question

In the laboratory a student uses a "coffee cup" calorimeter to
determine the specific heat of a metal.

She heats **19.5** grams of **tungsten**
to **97.80**°C and then drops it into a cup containing
**78.3** grams of water at **22.58**°C.
She measures the final temperature to be
**23.20**°C.

Assuming that all of the heat is transferred to the water, she
calculates the specific heat of **tungsten** to
be J/g°C.

Answer #1

A)In the laboratory a student uses a "coffee cup" calorimeter to
determine the specific heat of a metal.
She heats 19.3 grams of chromium
to 98.47°C and then drops it into a cup containing
81.8 grams of water at 23.17°C.
She measures the final temperature to be
24.97°C.
Assuming that all of the heat is transferred to the water, she
calculates the specific heat of chromium to be
__________________ J/g°C.
B) An electric range burner weighing 616.0
grams is turned...

In the laboratory a "coffee cup" calorimeter, or constant
pressure calorimeter, is frequently used to determine the specific
heat of a solid, or to measure the energy of a solution phase
reaction.
A student heats 60.93 grams of gold to 98.87 °C and then drops it
into a cup containing 79.68 grams of water at 24.46 °C. She
measures the final temperature to be 26.11 °C.
The heat capacity of the calorimeter (sometimes referred to as the
calorimeter constant) was...

In the laboratory a "coffee cup" calorimeter, or constant
pressure calorimeter, is frequently used to determine the specific
heat of a solid, or to measure the energy of a solution phase
reaction. Since the cup itself can absorb energy, a separate
experiment is needed to determine the heat capacity of the
calorimeter. This is known as calibrating the calorimeter and the
value determined is called the calorimeter constant. One way to do
this is to use a common metal of...

two parts for one question
-----------------------------------------
In the laboratory a "coffee cup" calorimeter, or constant
pressure calorimeter, is frequently used to determine the specific
heat of a solid, or to measure the energy of a solution phase
reaction. Since the cup itself can absorb energy, a separate
experiment is needed to determine the heat capacity of the
calorimeter. This is known as calibrating the calorimeter and the
value determined is called the calorimeter constant. One way to do
this is...

In the laboratory a
"coffee cup" calorimeter, or constant
pressure calorimeter, is frequently used to determine the specific
heat capacity of a solid, or to measure the enthalpy of a solution
phase reaction.
Since the cup itself can absorb energy, a separate experiment is
needed to determine the heat capacity of the calorimeter. This is
known as calibrating the calorimeter and
the value determined is called the calorimeter
constant.
One way to do this is to use a common metal...

In the laboratory a "coffee cup" calorimeter, or constant
pressure calorimeter, is frequently used to determine the specific
heat of a solid, or to measure the energy of a solution phase
reaction. A chunk of zinc weighing 18.01 grams and originally at
98.77 °C is dropped into an insulated cup containing 83.17 grams of
water at 20.02 °C. The heat capacity of the calorimeter (sometimes
referred to as the calorimeter constant) was determined in a
separate experiment to be 1.56...

A student wishes to determine the heat capacity of a coffee-cup
calorimeter. After she mixes 95.8 g of water at 62°C with 95.8 g of
water, already in the calorimeter, at 18.2°C, the final temperature
of the water is 35.0°C. Calculate the heat capacity of the
calorimeter in J/K. Use 4.184 J/g°C as the specific heat of
water.

In the laboratory a student heats 93.67 grams of lead to 98.92
°C and then drops it into a cup containing 83.45 grams of water at
21.01 °C. She measures the final temperature to be 24.18 °C.
calculate the calorimeter constant.

A student determines the heat of dissolution of solid
ammonium bromide using a coffee-cup calorimeter of
negligible heat capacity.
When 6.34 g of
NH4Br(s) is dissolved in
119.00 g of water, the temperature of the solution
drops from 25.00 to 22.76 °C.
Based on the student's observation, calculate the enthalpy of
dissolution of NH4Br(s) in kJ/mol.
Assume the specific heat of the solution is 4.184 J/g°C.
ΔHdissolution = kJ/mol

In the following experiment, a coffee-cup calorimeter containing
100. mL of H2O is used. The initial temperature of the calorimeter
is 23.0 ∘C. If 2.00 g of CaCl2 is added to the calorimeter, what
will be the final temperature of the solution in the calorimeter?
The heat of solution, ΔHsoln, of CaCl2 is −82.8 kJ/mol. The
specific heat of water is CS=4.184 J/(g−K

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