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Heat of Combustion Mass of water = 100g Temp rise of water = 15.0 C Mass of fuel used = 1.34g Molar mass of fuel = 56.4 g mol -1 Energy (Q) = mc T C =

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Presentation on theme: "Heat of Combustion Mass of water = 100g Temp rise of water = 15.0 C Mass of fuel used = 1.34g Molar mass of fuel = 56.4 g mol -1 Energy (Q) = mc T C ="— Presentation transcript:

1 Heat of Combustion Mass of water = 100g Temp rise of water = 15.0 C Mass of fuel used = 1.34g Molar mass of fuel = 56.4 g mol -1 Energy (Q) = mc T C = 4.18 J g -1 K -1 Molar heat of combustion = ?

2 Heat of Combustion Mass of water = 100g Temp rise of water = 15.0 C Mass of fuel used = 1.34g Molar mass of fuel = 56.4 g mol -1 Energy (Q) = mc T C = 4.18 J g -1 K -1 Energy absorbed by water (Q) = 100 x 15 x 4.18 = Moles fuel = 1.34 / 56.4 = Molar heat of combustion = 6270 / = ?

3 Heat of Combustion Mass of water = 100g Temp rise of water = 15.0 C Mass of fuel used = 1.34g Molar mass of fuel = 56.4 g mol -1 Energy (Q) = mc T C = 4.18 J g -1 K -1 Energy absorbed by water (Q) = 100 x 15 x 4.18 = Moles fuel = 1.34 / 56.4 = Molar heat of combustion = 6270 / = X

4 Heat of Combustion Mass of water = 100g Temp rise of water = 15.0 C Mass of fuel used = 1.34g Molar mass of fuel = 56.4 g mol -1 Energy (Q) = mc T C = 4.18 J g -1 K -1 Energy absorbed by water (Q) = 100 x 15 x 4.18 = Moles fuel = 1.34 / 56.4 = Molar heat of combustion = 6270 / = NO UNITS

5 Heat of Combustion Mass of water = 100g Temp rise of water = 15.0 C Mass of fuel used = 1.34g Molar mass of fuel = 56.4 g mol -1 Energy (Q) = mc T C = 4.18 J g -1 K -1 Energy absorbed by water (Q) = 100 x 15 x 4.18 = 6270 J Moles fuel = 1.34 / 56.4 = mol Molar heat of combustion = 6270 / mol = kJ mol -1 ?

6 Heat of Combustion Mass of water = 100g Temp rise of water = 15.0 C Mass of fuel used = 1.34g Molar mass of fuel = 56.4 g mol -1 Energy (Q) = mc T C = 4.18 J g -1 K -1 Energy absorbed by water (Q) = 100 x 15 x 4.18 = 6270 J Moles fuel = 1.34 / 56.4 = mol Molar heat of combustion = 6270 / mol = kJ mol -1 STILL NO UNITS X

7 Heat of Combustion Mass of water = 100g Temp rise of water = 15.0 C Mass of fuel used = 1.34g Molar mass of fuel = 56.4 g mol -1 Energy (Q) = mc T C = 4.18 J g -1 K -1 Energy absorbed by water (Q) = 100g x 15K x 4.18Jg -1 K -1 = 6270 J Moles fuel = 1.34g / 56.4 g mol -1 = mol Molar heat of combustion = 6270 J / mol = kJ mol -1 ?

8 Heat of Combustion Mass of water = 100g Temp rise of water = 15.0 C Mass of fuel used = 1.34g Molar mass of fuel = 56.4 g mol -1 Energy (Q) = mc T C = 4.18 J g -1 K -1 Energy absorbed by water (Q) = 100g x 15K x 4.18Jg -1 K -1 = 6270 J Moles fuel = 1.34g / 56.4 g mol -1 = mol Molar heat of combustion = 6270 J / mol = kJ mol -1 Wrong Significant Figures X

9 Heat of Combustion Mass of water = 100g Temp rise of water = 15.0 C Mass of fuel used = 1.34g Molar mass of fuel = 56.4 g mol -1 Energy (Q) = mc T C = 4.18 J g -1 K -1 Energy absorbed by water (Q) = 100g x 15K x 4.18Jg -1 K -1 = 6270 J Moles fuel = 1.34g / 56.4 g mol -1 = mol Molar heat of combustion = 6270 J / mol = 273 kJ mol -1 ?

10 Heat of Combustion Mass of water = 100g Temp rise of water = 15.0 C Mass of fuel used = 1.34g Molar mass of fuel = 56.4 g mol -1 Energy (Q) = mc T C = 4.18 J g -1 K -1 Energy absorbed by water (Q) = 100g x 15K x 4.18Jg -1 K -1 = 6270 J Moles fuel = 1.34g / 56.4 g mol -1 = mol Molar heat of combustion = 6270 J / mol = 264 kJ mol -1 Rounded before the end X

11 Heat of Combustion Mass of water = 100g Temp rise of water = 15.0 C Mass of fuel used = 1.34g Molar mass of fuel = 56.4 g mol -1 Energy (Q) = mc T C = 4.18 J g -1 K -1 Energy absorbed by water (Q) = 100g x 15K x 4.18Jg -1 K -1 = 6270 J Moles fuel = 1.34g / 56.4 g mol -1 Molar heat of combustion = 6270 J = 264 kJ mol g / 56.4 g mol -1 ?

12 Heat of Combustion Mass of water = 100g Temp rise of water = 15.0 C Mass of fuel used = 1.34g Molar mass of fuel = 56.4 g mol -1 Energy (Q) = mc T C = 4.18 J g -1 K -1 Energy absorbed by water (Q) = 100g x 15K x 4.18Jg -1 K -1 = 6270 J Moles fuel = 1.34g / 56.4 g mol -1 Molar heat of combustion = 6270 J = 264 kJ mol g / 56.4 g mol -1 Much Better !


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