Question

Calculate heat of combustion reaction of 1.0 g of octane:

2 C8H18 + 25 O2 --> 16 CO2 + 18 H2O

The calorimeter contains 1200 g water, and the temperature changes from 25.00 deg C to 33.20 deg C. Heat capacity of bomb is 837 J/deg C.

Answer #1

**Answer** – We are given, mass of octane = 1.0
g

Mass of water = 1200 g , ti = 25.0 ^{o}C, tf = 33.20
^{o}C, Heat capacity of bomb = 837 J/^{o}C

Reaction - 2 C_{8}H_{18} + 25 O_{2}
----> 16 CO_{2} + 18 H_{2}O

We know the, heat of combustion reaction = heat of water + heat of bomb calorimeter

First we need to calculate the heat absorbed by water and bomb calorimeter

Heat of water and we know formula

Heat, q = m*C*∆t

= 1200 g * 4.184 J/g^{o}C. * ( 33.20 –
25.0)^{o}C

= 41170.6 J

Heat of bomb calorimeter

Heat, q = C * ∆t

= 837 J/^{o}C * ( 33.20 – 25.0)^{o}C

= 6863.4 J

So –q_{rxn} =q for water + q for colorimeter

= 41170.6 + 6863.4 J

= 48033.96 J

q_{rxn} =-
48.034 kJ

Moles of octane = 1.0 g / 114.23 g.mol^{-1}

= 0.00875 moles

So, **heat of combustion reaction** = -48.0 kJ /
0.00875 moles

= **- 5.49*10 ^{3} kJ/mol**

A 1.00 g sample of octane (C8H18) is burned in a calorimeter
that contains 1.20 kg of water. The temperature of the water and
the bomb rises from 25.00°C to 33.20°C. The heat capacity of the
bomb, Cbomb, is 837 J/0C . Specific heat for water: 4.184
Jg–1°C–1.
a) Calculate the amount of heat gained by the calorimeter
b) Calculate the amount of heat gained by the water
c) Calculate the amount of heat given off per mol of octane...

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
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Question 4
Part A
Using the following equation for the combustion of octane,
calculate the heat of reaction for 100.0 g of octane. The molar
mass of octane is 114.33 g/mole.
2 C8H18 + 25 O2 → 16
CO2 + 18 H2O ΔH°rxn = -11018
kJ
Using the following equation for the combustion of octane,
calculate the heat of reaction for 100.0 g of octane. The molar
mass of octane is 114.33 g/mole.
2 C8H18 + 25 O2 → 16...

Using the following equation for the combustion of octane,
calculate the heat of reaction for 100.0 g of octane. The molar
mass of octane is 114.33 g/mole.
2 C8H18 + 25 O2 -> 16 CO2 + 18 H2O ,deltaH°rxn =
-11018 kJ
I got- 4820kJ but the answer is 4820kJ.
why is the answer positive when the delta h is negative?

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The combustion of titanium with oxygen produces titanium
dioxide: Ti (s) + O2(g) → TiO2 (s) When 2.060 g of titanium is
combusted in a bomb calorimeter, the temperature of the calorimeter
increases from 25.00 °C to 91.60 °C. In a separate experiment, the
heat capacity of the calorimeter is measured to be 9.84 kJ/K. The
heat of reaction for the combustion of a mole of Ti in this
calorimeter is ________ kJ/mol.

The combustion of titanium with oxygen produces titanium
dioxide:
Ti (s) + O2 (g) → TiO2 (s)
When 2.060 g of titanium is combusted in a bomb calorimeter, the
temperature of the calorimeter increases from 25.00 °C to 91.60 °C.
In a separate experiment, the heat capacity of the calorimeter is
measured to be 9.84 kJ/K. The heat of reaction for the combustion
of a mole of Ti in this calorimeter is __________ kJ/mol.
Ti = 47.867 amu
O2 =...

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...

Here is the combustion reaction for octane (C8H18), which is a
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1.) In an experiment, a 0.6319 g sample of
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During the combustion the temperature increases from
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capacity of water is 4.184 J g-1°C-1.
The heat capacity of the calorimeter was determined in a previous
experiment to be 786.6 J/°C.
Assuming that no energy is lost to the surroundings, calculate the
molar heat of combustion of
para-benzoquinone...

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