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21 May, 08:39

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. Write the balanced chemical equation for the reaction in the calorimeter. How many joules were liberated by the reaction? How many joules would be liberated under similar conditions if 1.000 mol of toluene was burned?

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  1. 21 May, 11:15
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    There were 63.67 kJ liberated

    If 1 mol of toluene was burned, there would be liberated 3906 kJ / mole

    Explanation:

    Step 1: Data given

    Mass of the toluene sample = 1.500 grams

    The temperature of the calorimeter rose from 25.000 °C to 26.413 °C

    Write the balanced chemical equation for the reaction in the calorimeter.

    C7H8 (l) + 9O2 (g) ⇒ 7CO2 (g) + 4H2O (l)

    Step 2: Calculate Q of the calorimeter

    Q = C * Δt

    Q = 45.06 kJ / °C * (26.413 - 25)

    Q = 63.67 kJ

    Step 3: Calculate moles of toluene

    Moles toluene = mass toluene / molar mass toluene

    Moles toluene = 1.500 grams / 92.14 g/mol

    Moles toluene = 0.0163 moles

    Step 4: Calculate energy per mole

    energy per mole = 63.67 kJ / 0.0163 moles = 3906 kJ / mole
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