a) Toluene, C7H8, is used in the manufacture of explosives such as TNT (trinitrotoluene). A 1.500 g sample of liquid toluene was placed in a bomb calorimeter along with excess oxygen. When the combustion of the toluene was initiated, the temperature of the calorimeter rose from 25.000 °C to 26.413 °C. The products of the combustion are CO2(g) and H2O(l), and the heat capacity of the calorimeter was 45.06 kJ °C-1.
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1) Write the balanced chemical equation for the reaction int he calorimeter
2) How many kilojoules were liberated by the reaction?
3)How many joules would be liberated under similar conditions if 1.000 mol of toluene were burned? For scientific notation, use 1.00E08, for example.
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b) Methanol is the fuel in "canned heat" containers (e.g., Sterno) that are used to heat food at cocktail parties. The combustion of methanol follows the thermochemical equation:
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2CH3OH(l) + 3O2(g) → 2CO2(g) + 4H2O(l) ΔH° = -1199 kJ
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How many kilojoules are liberated by the combustion of 58.4 g of methanol?
Answers
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Posted 27 Apr 2017 08:04 AM
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