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21 February, 03:13

When methanol, CH 3 OH, is burned in the presence of oxygen gas, O 2, a large amount of heat energy is released. For this reason, it is often used as a fuel in high performance racing cars. The combustion of methanol has the balanced, thermochemical equation

CH3OH (g) + 3/2O2 (g) ⟶ CO2 (g) + 2H2O (I) Δ H = - 764 kJ.

How much methanol, in grams, must be burned to produce 575 kJ of heat?

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  1. 21 February, 03:35
    0
    24.1 g

    Explanation:

    Let's consider the following thermochemical equation.

    CH₃OH (g) + 3/2 O₂ (g) ⟶ CO₂ (g) + 2 H₂O (I) ΔH = - 764 kJ

    In order to produce 764 kJ of heat, 1 mole of methanol must be burned. To produce 575 kJ, the required moles of methanol are:

    -575 kJ * (1 mol CH₃OH / - 764 kJ) = 0.753 mol CH₃OH

    The molar mass of methanol is 32.04 g/mol. 0.753 moles of methanol represent a mass of:

    mass = moles * molar mass

    0.753 mol * (32.04 g/mol) = 24.1 g
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