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
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Specific heat of water is 4.184 J/gC. Answer to 0 decimal places
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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?

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 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
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(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

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
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these data, calculate the heat of combustion of naphthalene in
kJ/mol.

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