Question

A 2.50 mol sample of benzene (C6H6, 78.11 g/mol) was burned in a bomb calorimeter with a heat capacity of 800 J/°C. The calorimeter contained 100g of water (4.18J/g°C) and the temperature increased by 4°C. What is the molar enthalpy of combustion for this compound?

Answer #1

heat absorbed by calorimeter = heat capacity * temperature change

= 800*4 = 32000joules

heat absorbed by water = mcT

= 100*4.18*4 = 1672 joules

total heat = 32000+1672 = 33672 joules = 33.672 kj

total heat divide by 2.5 moles of benzen = 33.672/2.5 = 13.4688kj/mole

A 1.000g sample of benzene (C6H6) is
burned in a bomb calorimeter whose total heat capacity is 4.957 kJ/
oC. If the temperature of the calorimeter increases from
25.30 to 33.74 oC , what is the heat of combustion of
the benzene per mole.
Explanation please.

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.

When 1.020 g of ethanol (C2H6O, 46.07 g/mol) was burned in a
bomb calorimeter containing 2400. g of water, the temperature of
the water rose from 22.46 to 25.52ºC. The specific heat
of water is 4.18 J/g-°C. What is the enthalpy of combustion of 1
mol of ethanol? What is the heat capacity of the calorimeter?

A 5.00g sample of TNT (C7H5N2O6) is burned in a bomb calorimeter
with a heat capacity of 420 J/ºC. The calorimeter contained 610
grams of water (4.18J/gºC) and the temperature of the water was
measured to go from 20.0 ºC to 22.5 ºC. What is the heat of
combustion of TNT?
(1) -79.10 kJ/mol (2) -158.2 kJ/mol (3) -258.2 kJ/mol (4) -316.5
kJ/mol (5) -632.9 kJ/mol

1 g of C6H6(l) (benzene) is burned in an adiabatic bomb
calorimeter (constant volume). T before ignition was 20.826 °C and
25.000 °C after combustion (remember that the energy change of the
bomb is opposite the energy change of the combustion). The heat
capacity of the calorimeter was 10.000 kJ K-1. Calculate fHm for
benzene at 298.15 K from this data (make sure to convert your
enthalpies to molar values). Use the tables in the back of the book
(resource...

A 0.553-g sample of diphenyl
phthalate
(C20H14O4) is
burned in a bomb calorimeter and the temperature increases from
24.40 °C to 27.57 °C. The
calorimeter contains 1.08×103 g of
water and the bomb has a heat capacity of 877
J/°C. The heat capacity of water is 4.184 J
g-1°C-1. Based on this experiment, calculate
ΔE for the combustion reaction per mole of diphenyl
phthalate burned.
______ 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).

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 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.

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