Question

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 8.70 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.

Answer #1

Molecular weight of CaCl2= 8.7 gm

Moles of CaCl2= mass/Molecular weight , Molecular weight of CaCl2= 111 gms

Moles of CaCl2= 8.7/111=0.0783 moles

Mass of water =100*1 =100 gm ( density of water = 1 gm/cc)

Mass of solution = mass of water + mass of CaCl2= 100+8.7= 108.7 gms

heat of solution = -82.8 Kj/mol

1mol of CaCl2 gives rise to 82.8 Kj= 82.8*1000 joules=82800 joules

0.0783 moles give rise to 0.0783*82800 joules=6483.24joules

Cp = specific heat of solution , same as that of water= 4.184, m =mass of solution, delT= temperature difference

From mCpdelT= 6483.24

108.7*4.184*delT)= 6483.24

delT= 6483.24/(108.7*4.184)=14.25

T- 23 =14.25 , T = 37.25 deg.c

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 2.60 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.

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 8.10 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.

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 9.70 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.

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 3.50 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.

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 5.20 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. Express your
answer with the appropriate units.

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

A coffee-cup calorimeter containing 100 mL of H2O is used. The
initial temperature of the calorimeter is 23.0 ∘C. If 9.00 g of
CaCl2 is added to the calorimeter, what will be the final
temperature (in ∘C ) of the solution in the calorimeter? The heat
of solution ΔHsoln of CaCl2 is −82.8 kJ/mol.

Part A
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 2.60 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.
Express your answer with the appropriate units.

In a coffee-cup calorimeter experiment, 10.00 g of a soluble
ionic compound was added to the calorimeter containing 75.0 g H2O
initially at 23.2°C. The temperature of the water increased to
31.8°C. What was the change in enthalpy for the dissolution of the
compound? Give your answer in units of joules per gram of compound.
Assume that the specific heat of the solution is the same as that
of pure water, 4.18 J ⁄ (g ⋅ °C).

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...

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