Question
In: Chemistry
In an adiabatic, constant-volume bomb calorimeter, a combustion of 0.7362g of naphthalene (C10H8) caused the temperature...
In an adiabatic, constant-volume bomb calorimeter, a combustion of 0.7362g of naphthalene (C10H8) caused the temperature to rise of 5.707 Celcius. The final temperature was 298.000K. The heat capacity of the calorimeter, Ccal was 10290 J/K . (Note: this value of Ccal includes the contribution from water.) The molar enthalpies of formation of CO2(g) and H2O(l) are: -393.522 kJ/mol, -285.830 kJ/mol, respectively Mm(C)= 12.01 g/mol and Mm(H)= 1.001 g/mol.
a.) Calculate deltaUc , deltaUcm , delta Hcm for this combustion reaction.
b.) What are delta Hf and delta Hfm of naphthalene?
Solutions
Expert Solution
Note: FYI, the values
calculated here do not agree with the actual scientific data. There
must be some error in either temperature rise(5.707) or the heat
capacity of the calorimeter.
queen_honey_blossom answered 7 months agoRelated Solutions
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ΔΔ
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What is the energy change associated with 3.5 mol of
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⟶⟶
⟶⟶ D + E ...
A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat...
A bomb calorimeter, or constant volume calorimeter, is a device
often used to determine the heat of combustion of fuels and the
energy content of foods. Since the "bomb" itself can absorb energy,
a separate experiment is needed to determine the heat capacity of
the calorimeter. This is known as calibrating the calorimeter. In
the laboratory a student burns a 0.466-g sample of 1,8-octanediol
(C8H18O2) in a bomb calorimeter containing 1200. g of water. The
temperature increases from 25.90 °C...
1.A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the...
1.A bomb calorimeter, or a constant volume calorimeter, is a
device often used to determine the heat of combustion of fuels and
the energy content of foods. In an experiment, a 0.3807 g sample of
1,6-hexanediol (C6H14O2) is burned completely in a bomb
calorimeter. The calorimeter is surrounded by 1.139×103 g of water.
During the combustion the temperature increases from 25.30 to 27.59
°C. The heat capacity of water is 4.184 J g-1°C-1. The heat
capacity of the calorimeter was...
A)A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat...
A)A bomb calorimeter, or constant
volume calorimeter, is a device often used to determine the heat of
combustion of fuels and the energy content of foods.
Since the "bomb" itself can absorb energy, a separate experiment is
needed to determine the heat capacity of the calorimeter. This is
known as calibrating the
calorimeter.
In the laboratory a student burns a 0.392-g sample
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(C15H16O2) in a
bomb calorimeter containing 1140. g of water. The
temperature increases from 25.00...
A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat...
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often used to determine the heat of combustion of fuels and the
energy content of foods. Since the "bomb" itself can absorb energy,
a separate experiment is needed to determine the heat capacity of
the calorimeter. This is known as calibrating the calorimeter. In
the laboratory a student burns a 0.337-g sample of bisphenol A
(C15H16O2) in a bomb calorimeter containing 1040. g of water. The
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When 0.595 g of biphenyl (C12H10) undergoes combustion in a bomb calorimeter, the temperature rises from...
When 0.595 g of biphenyl (C12H10) undergoes combustion in a bomb
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Part A
Find ΔErxn for the combustion of biphenyl in kJ/mol biphenyl.
The heat capacity of the bomb calorimeter, determined in a separate
experiment, is 5.86 kJ/∘C.
Part B
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a) Calculate ΔU∘f for K2O.
b) Calculate ΔH∘f for K2O.
the answer for ΔU∘f = -362 kJ⋅mol−1
and for ΔH∘f =
-363 kJ⋅mol−1
how they got that answers ????
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from 18.43 °C to 35.02 °C. Calculate the heat of combustion (in
kJ/g) of the hydrogen. Report your answer to three significant
figures.
Please show your work and equations. Thank
you!
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