Question

A **0.553**-g sample of **diphenyl
phthalate**
(**C _{20}H_{14}O_{4}**) is
burned in a bomb calorimeter and the temperature increases from

______ kJ/mol

Answer #1

The heat given by combustion = heat absorbed by bomb calorimeter + heat absorbed by water

Thus

heat absorbed by bomb = heat capacity x differenc ein temperature

= 877J /C x 3.17C

= 2780.09 J

heat absorbed by water = mass x specific heat x difference in temperature

= 1.08x 10^{3} gx 4.18 J/g.C x3.17C

= 14310.648 J

Total heat given in combustion = 2780.09 J + 14310.648 J

= 17090.738 J

molar mass of diethyl pthalate = 318g/mol

Thus if 0.533 g sample on combustion gives 17090.738 J

1 mol (318g) sample on combustion can give = 318g /molx 17090.738 J/0.533g

=10196725 J

= 10196.73 kJ/mol

Thus the delta E of combustion of mole of diphenylphthalate = 10196.73 kJ/mol

A 0.373-g sample of naphthalene (C10H8) is burned in a bomb
calorimeter and the temperature increases from 24.90 °C to 27.80
°C. The calorimeter contains 1.05E3 g of water and the bomb has a
heat capacity of 836 J/°C. Based on this experiment, calculate ΔE
for the combustion reaction per mole of naphthalene burned
(kJ/mol).

A 0.287-g sample of bianthracene (C28H18) is burned in a bomb
calorimeter and the temperature increases from 25.30 °C to 27.50
°C. The calorimeter contains 1.03E3 g of water and the bomb has a
heat capacity of 856 J/°C. Based on this experiment, calculate ΔE
for the combustion reaction per mole of bianthracene burned
(kJ/mol).

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 0.4137 g sample of
bianthracene
(C28H18) is burned
completely in a bomb calorimeter. The calorimeter is surrounded by
1.361×103 g of water. During the
combustion the temperature increases from 24.82 to
27.25 °C. The heat capacity of water is 4.184 J
g-1°C-1.
The heat capacity of the calorimeter...

A 12.8 g sample of ethanol (C2H5OH) is
burned in a bomb calorimeter with a heat capacity of 5.65
kJ/°C. The temperature of the calorimeter and the contents
increases from 25°C to 35°C. What is the heat of
combustion per mole of ethanol? The molar mass of ethanol is 46.07
g/mol.
C2H5OH (l) + 3 O2 (g) -----> 2 CO2 (g) + 3
H2O (g) ΔE = ?

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 1.4170 g sample of
L-ascorbic acid
(C6H8O6) is
burned completely in a bomb calorimeter. The calorimeter is
surrounded by 1.354×103 g of water.
During the combustion the temperature increases from
24.92 to 27.68 °C. The heat
capacity of water is 4.184 J g-1°C-1.
The heat capacity of the calorimeter...

A 1.000 g sample of octane (C8H18) is burned in a bomb
calorimeter containing 1200 grams of water at an initial
temperature of 25.00ºC. After the reaction, the final temperature
of the water is 33.20ºC. The heat capacity of the calorimeter (also
known as the “calorimeter constant”) is 837 J/ºC. The specific heat
of water is 4.184 J/g ºC. Calculate the heat of combustion of
octane in kJ/mol.

A 1.00g sample of octane (C8H18) is burned in a calorimeter that
contains 1.20kg of water. The temperature of the water and the bomb
rises from 25.00oC to 33.20oC. If the heat capacity of the bomb,
Cbomb, is 837J/K calculate the heat given off per mole of octane.
Specific heat for water: 4.184 J/g.°C
Please show work, correct equation to use and values. I know how
to calculate heat but not sure how to correctly find heat per
mole.
86...

. A 0.500 g sample of naphthalene (C10H8) is burned in a bomb
calorimeter containing 650 grams of water at an initial temperature
of 20.00 oC. After the reaction, the final temperature of the water
is 26.4ºC. The heat capacity of the calorimeter is 420 J/oC. Using
these data, calculate the heat of combustion of naphthalene in
kJ/mol.

A 3.250g sample of methanol, CH3OH, is combusted un a bomb
calorimeter. The temperature of the calorimeter increases by 12.55
degrees celsius. If the heat capacity of the bomb is 850.0
J/degrees celsius and it contains 1.200kg of water, what is the
heat envolved per mole of ethanol combusted? The specific heat
capaacity of water is 4.184 J/g degrees celsius and the molar mass
of methanol is 32.04g/mol.

When 86.6 g of a compound was burned in a bomb calorimeter that
contained 0.184 kg of water the temperature rise of the water in
the calorimeter was 57.0C. If the heat of combustion of the
compound is 1,396 kJ/mol, what is the molar mass of the compound?
Specific heat of water is 4.184 J/gC. Answer to 0 decimal places
and enter the units.

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