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Heat of Combustion Lab Research Assignment Paper (Multiple Choice Questions Sample)
Instructions:
Answer the following equations from heat of combustions
source..Content:
Students Name
Professor’s Name
Course
Date
Heat of Combustion Lab
Introduction
1. You may recall that the products of the complete combustion of a Hydrocarbon are water vapor and carbon dioxide gas. Write the balanced equation showing the combustion of methane. Do not forget to include the states of matter of the reactants and the products. Hint: Methane is a gas at standard temperature and pressure.
CH4 (g) +2O2 (g) в†’ CO2 (g) +2H2O (l)
To begin the experiment, 1.11g of methane CH4 is burned in a bomb calorimeter containing 1000 grams of water. The initial temperature of water is 24.85o C .The specific heat of water is 4.184 J/g .oC. The heat capacity of the calorimeter is 695 J/ oC. After the reaction the final temperature of the water is 35.65oC.
2. Calculate the change in temperature, О”T
О”T= (t2-t1)0c
= (35.65-24.85)0C
=10.800C
3. Using the formula water q =m•c• ΔT, calculate the heat absorbed by the water
Q water = m•c• ΔT
= 1000g•4.184J/g.0C•10.800C
= -45187.2Joules
4. Using the formula cal q =C • ΔT, calculate the heat absorbed by the Calorimeter.
Q calorimeter = C calorimeter• ΔT
= 695J/0C•10.800C
= -7506 Joules
5. The total heat absorbed by the water and the calorimeter can be calculated by adding the heat calculated in steps 3 and 4.
Total heat released during combustion = Q calorimeter+ Q water
= - (45187.2+7506) Joules
= -52693.2 Joules
в‰…-52.6932KJ
The amount of heat released by the reaction is equal to the amount of heat absorbed with the negative
Sign as this is an exothermic reaction. Using the formula ∆H = - (qcal+ qwater), calculate the total heat of combustion.
Molar mass of CH4 is 16.04g/mol, therefore calculating number of moles,
1.11g of CH4 (methane) releases 52.6932KJ, therefore for one mole (16.04g/mole), the amount of heat released is;
= (- 52.6932KJ•16.04g/mol)/1.11g
= -761.4405KJ/mole
Therefore the experimental molar heat of combustion of more or less heat of combustion of methane is -761.4405KJ/mole.
6. Evaluate the information contained in this calculation and complete the
Following sentence:
This calculation shows that burning __1.11_ grams of methane [takes
In/gives off] _761.4405KJ/mole _energy.
...
Professor’s Name
Course
Date
Heat of Combustion Lab
Introduction
1. You may recall that the products of the complete combustion of a Hydrocarbon are water vapor and carbon dioxide gas. Write the balanced equation showing the combustion of methane. Do not forget to include the states of matter of the reactants and the products. Hint: Methane is a gas at standard temperature and pressure.
CH4 (g) +2O2 (g) в†’ CO2 (g) +2H2O (l)
To begin the experiment, 1.11g of methane CH4 is burned in a bomb calorimeter containing 1000 grams of water. The initial temperature of water is 24.85o C .The specific heat of water is 4.184 J/g .oC. The heat capacity of the calorimeter is 695 J/ oC. After the reaction the final temperature of the water is 35.65oC.
2. Calculate the change in temperature, О”T
О”T= (t2-t1)0c
= (35.65-24.85)0C
=10.800C
3. Using the formula water q =m•c• ΔT, calculate the heat absorbed by the water
Q water = m•c• ΔT
= 1000g•4.184J/g.0C•10.800C
= -45187.2Joules
4. Using the formula cal q =C • ΔT, calculate the heat absorbed by the Calorimeter.
Q calorimeter = C calorimeter• ΔT
= 695J/0C•10.800C
= -7506 Joules
5. The total heat absorbed by the water and the calorimeter can be calculated by adding the heat calculated in steps 3 and 4.
Total heat released during combustion = Q calorimeter+ Q water
= - (45187.2+7506) Joules
= -52693.2 Joules
в‰…-52.6932KJ
The amount of heat released by the reaction is equal to the amount of heat absorbed with the negative
Sign as this is an exothermic reaction. Using the formula ∆H = - (qcal+ qwater), calculate the total heat of combustion.
Molar mass of CH4 is 16.04g/mol, therefore calculating number of moles,
1.11g of CH4 (methane) releases 52.6932KJ, therefore for one mole (16.04g/mole), the amount of heat released is;
= (- 52.6932KJ•16.04g/mol)/1.11g
= -761.4405KJ/mole
Therefore the experimental molar heat of combustion of more or less heat of combustion of methane is -761.4405KJ/mole.
6. Evaluate the information contained in this calculation and complete the
Following sentence:
This calculation shows that burning __1.11_ grams of methane [takes
In/gives off] _761.4405KJ/mole _energy.
...
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