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 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

Answer #1

given the mass of CaCl2 = 2.00 g

molecular mass of CaCl2 = 111.0 g/mol

Hence moles of CaCl2 = 2.00 g / 111.0 g/mol = 0.01802 mol

Given ΔHsoln = - 82.8 KJ/mol (exothermic)

Hence the amount of heat liberated by 2.00 g of CaCl2 = (- 82.8 KJ/mol) x 0.01802 mol = 1.492 KJ = 1492 J

Hence heat accepted by water = 1492 J

mass of water = 100.0 mL x 1g/mL = 100 g

Let the final temperature be 'T' DegC

=> mxSxT = 1492 J

=> 100 g x 4.184 J/(g−C) x (T - 23.0) = 1492 J

=> T - 23.0 = 3.566

=> T = 26.566 DegC (answer)

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 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.

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.

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).

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

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