Question

A student dissolves 5g of NaOH in 100mL of water at 25.0
^{o}C in a calorimeter. The final temperature of the
solution was found to be 35.4 ^{o}C. Assume the calorimeter
constant is 92J/^{o}C , the density of the solution is
1g/ml, and the specific heat of the solution is 4.184J/g
^{o}C. Calculate the enthalpy of solution of NaOH in kJ/mol
NaOH.

Answer #1

A student mixes 100mL of 0.5M NaOH and 100mL of 0.5M HCl at 25.0
oC in a calorimeter. The final temperature of the
solution was found to be 28.02 oC. Assume the
calorimeter constant is 92J/oC , the density of the
solution is 1g/ml, and the specific heat of the solution is
4.184J/g oC. Calculate the enthalpy of neutralization
NaOH(aq) in kJ/mol NaOH.

1.
When a solid dissolves in water, heat may be evolved or
absorbed. The heat of dissolution
(dissolving) can be determined using a coffee cup
calorimeter.
In the laboratory a general chemistry student finds that when
6.20 g of CsClO4(s)
are dissolved in 115.60 g of water, the
temperature of the solution drops from
22.87 to 19.50 °C.
Based on the student's observation, calculate the enthalpy of
dissolution of CsClO4(s) in
kJ/mol.
Assume the specific heat of the solution is...

Part A A calorimeter contains 25.0 mL of water at 11.5 ∘ C .
When 1.20 g of X (a substance with a molar mass of 73.0 g/mol ) is
added, it dissolves via the reaction X(s)+ H 2 O(l)→X(aq) and the
temperature of the solution increases to 30.0 ∘ C . Calculate the
enthalpy change, ΔH , for this reaction per mole of X . Assume that
the specific heat of the resulting solution is equal to that of...

When a solid dissolves in water, the solution may become hotter
or colder. The dissolution enthalpy (dissolving) can be determined
using a coffee cup calorimeter. In the laboratory a general
chemistry student finds that when 10.13 g K2SO4(s) is dissolved in
114.80 g water, the temperature of the solution drops from 24.11 to
20.86 °C. The heat capacity of the calorimeter (sometimes referred
to as the calorimeter constant) was determined in a separate
experiment to be 1.77 J/°C. Based on...

When a 5.93-g sample of solid sodium hydroxide dissolves in 39.8
g of water in a coffee-cup calorimeter (see above figure) the
temperature rises from 22.00 oC to 56.12 oC. Calculate H in kJ/mol
NaOH for the solution process. NaOH(s) Na+(aq) + OH-(aq) The
specific heat of water is 4.18 J/g-K.

A calorimeter contains 35.0 mL of water at 15.0 ∘C . When 1.70 g
of X (a substance with a molar mass of 76.0 g/mol ) is added, it
dissolves via the reaction
X(s)+H2O(l)→X(aq) and the
temperature of the solution increases to 25.0 ∘C .
Calculate the enthalpy change, ΔH, for this reaction
per mole of X.
Assume that the specific heat of the resulting solution is equal
to that of water [4.18 J/(g⋅∘C)], that density of water is 1.00...

Andrea has been measuring the enthalpy change associated with
reaction between HCl and NaOH in a coffee cup calorimeter. Andrea
combined 51.48 mL of 1.00 M HCl and 34.62 mL of 1.00 M NaOH in a
coffee cup calorimeter (mass of the coffee cups + a stir bar =
15.00 g). If the initial temperature of the acid/base solution was
17.13 oC, and the final observed temperature was 27.95 oC, what is
the enthalpy change of the neutralization reaction, in...

When a solid dissolves in water, heat may be evolved or
absorbed. The heat of dissolution
(dissolving) can be determined using a coffee cup
calorimeter.
In the laboratory a general chemistry student finds that when
18.53 g of
Cs2SO4(s) are dissolved in
100.40 g of water, the temperature of the solution
drops from 25.54 to
22.92 °C.
The heat capacity of the calorimeter (sometimes referred to as the
calorimeter constant) was determined in a separate
experiment to be 1.85 J/°C....

3. A sample of metal weighing 35.5g at a temperature of 100 oC
was placed in a calorimeter containing 50 g of water at 25.0 oC. At
equilibrium the temperature of water and metal was 35.5 oC.
Calculate the heat capacity of the metal. . Use this value for
Cp:27.65.
4. When 0.50 g of magnesium metal is placed in a calorimeter,
and 100. mL of 1.0 M HCl were added the temperature of solution
increased from 22.2 oC to...

Suppose that 300.0 mL of 1.00 M HCl at 25.0°C
is added to 300.0 mL of 1.00 M NaOH at 25.0°C in a coffee
cup calorimeter. If the enthalpy of the reaction is −54.0 kJ/mol of
NaCl formed, what is the final temperature of the solution in the
calorimeter? Assume the mixture has a specific heat capacity of
4.18 J/(g·K) and a density of 1.00 g/mL
(1)
3.5°C
(2) 6.5°C
(3)
18.5°C
(4)
31.5°C
(5) 46.5°C

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