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Published byAdrian Woodward Modified over 4 years ago

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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 = 4.18 J g -1 K -1 Molar heat of combustion = ?

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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 = 4.18 J g -1 K -1 Energy absorbed by water (Q) = 100 x 15 x 4.18 = 6270. Moles fuel = 1.34 / 56.4 = 0.023 Molar heat of combustion = 6270 / 0.023 = 272.6 ?

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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 = 4.18 J g -1 K -1 Energy absorbed by water (Q) = 100 x 15 x 4.18 = 6270. Moles fuel = 1.34 / 56.4 = 0.023 Molar heat of combustion = 6270 / 0.023 = 272.6 X

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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 = 4.18 J g -1 K -1 Energy absorbed by water (Q) = 100 x 15 x 4.18 = 6270. Moles fuel = 1.34 / 56.4 = 0.023 Molar heat of combustion = 6270 / 0.023 = 272.6 NO UNITS

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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 = 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 = 0.023 mol Molar heat of combustion = 6270 / 0.023 mol = 272.6 kJ mol -1 ?

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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 = 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 = 0.023 mol Molar heat of combustion = 6270 / 0.023 mol = 263.9 kJ mol -1 STILL NO UNITS X

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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 = 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 = 0.023 mol Molar heat of combustion = 6270 J / 0.023 mol = 272.6 kJ mol -1 ?

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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 = 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 = 0.023 mol Molar heat of combustion = 6270 J / 0.023 mol = 272.6 kJ mol -1 Wrong Significant Figures X

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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 = 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 = 0.023 mol Molar heat of combustion = 6270 J / 0.023 mol = 273 kJ mol -1 ?

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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 = 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 = 0.023 mol Molar heat of combustion = 6270 J / 0.023 mol = 264 kJ mol -1 Rounded before the end X

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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 = 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 -1 1.34g / 56.4 g mol -1 ?

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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 = 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 -1 1.34g / 56.4 g mol -1 Much Better !

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