Question

What is recorded as the final temperature (in oC) on a constant pressure calorimeter if 9.377 g of potassium hydroxide is dissolved in 30.431 mL of water originally at 21.094oC?

Answer #1

**enthalphy of solution for KOH = -57.61
KJ/mol**

**mass of KOH =**9.377 g

**Molar mass of KOH = 56.1 g/mol
number of moles of KOH = mass/ molar mass = 9.377/56.1 = 0.167
mol**

**Heat released = number of moles * enthalphy of solution
= 0.167*57.61 = 9.6 KJ = 9600 J**

**Specific heat capacity of water = 4.186 J/goC
mass of water = volume * density = 30.431 mL * 1 g/mL = 30.431
g**

**This heat is absorbed by water
Let final temperature be T oC
Q = m*C* delta T
9600 = 30.431 * 4.186 * (T- 21.094)
T-21.094 = 75.36
T=96.45 oC
Answer: 96.45 oC**

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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...

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...

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Calculate the heat capacity of the metal. . Use this value for
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X(s) ------ X(aq)
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A generic solid, X, has a molar mass of 67.9 g/mol. In a
constant-pressure calorimeter, 16.8 g of X is dissolved in 269 g of
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X(s) ------ X(aq)
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