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21 February, 18:08

Combustion of ethylene glycol leads to a change in internal energy (/DeltaU) of - 1189 kJ at 298 K. What is the corresponding change in enthalpy in kJ/DeltaH? HOCH_2CH_2OH (l) + 5/2 O_2 (g) → 2 CO_2 (g) + 3 H_2O (l) / DeltaU = - 1189 kJ

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  1. 21 February, 18:16
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    -1190.24 kJ

    Explanation:

    The enthalpy change in a chemical reaction that produces or consumes gases is given by the expression:

    ΔH = ΔU + Δngas RT

    where Δn gas is the change of moles of gas, R is the gas constant, and T is temperature.

    Now from the given balanced chemical reaction, the change in number of mol gas is equal to:

    Δn gas = mole gas products - mole gas reactants = 2 - 5/2 = - 1/2 mol

    Sionce we know ΔU and the temperature (298 K), we are in position to calculate the change in enthalpy.

    ΔH = - 1189 x 10³ J + (-0.5 mol) 8.314 J/Kmol x 298 K

    ΔH = - 1.190 x 10⁶ J = - 1.190 x 10⁶ J x 1 kJ/1000 J = - 1.190 x 10³ J
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