Question

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.

Answer #1

The number of moles of methanol combusted.

The temperature of the calorimeter increases by 12.55 degrees celsius. If the heat capacity of the bomb is 850.0 J/degrees celsius. The amount of heat gained by calorimeter

The mass of water

The specific heat capacity of water is 4.184 J/g degrees celsius. The temperature of increases by 12.55 degrees celsius

The amount of heat gained by water

Total heat

The heat evolved per mole of ethanol combusted

Convert the unit from J to kJ

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).

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 2.64 g sample of hydroquinone (C6H6O2) was combusted in a bomb
calorimeter. 234 joules of energy was generated. The temperature
rose from 25.0°C to 34.9°C. Calculate the heat capacity, molar heat
capacity and the specific heat capacity.

Part A
When 2.275 g of anthracene, C14H10, is
combusted in a bomb calorimeter that has a water jacket containing
500.0 g of water, the temperature of the water increases by
43.15°C. Assuming that the specific heat of water is 4.18 J/(g •
°C), and that the heat absorption by the calorimeter is negligible,
estimate the enthalpy of combustion per mole of anthracene.
Part B
The specific heat capacity of methane gas is 2.20 J/g• K. How
many joules of...

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...

When 2.25mg of anthracene was combusted in a constant volume
bomb calorimeter, the temperature rose by 1.35K. Given that the
standard molar enthalpy of combustion of anthracene at 298K is
-7061 kJ/mol, calculate the heat capacity of the calorimeter.

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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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