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    Standard Enthalpies of Reaction

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    50 g of C16H34 are burned with insufficient oxygen for complete combustion to CO2.
    C16H34(s) + 16.5 O2(g) -> 16 CO(g) + 17 H2O(l) and some of the reaction forms CO2 and H2O(l) in the reaction C16H34(s) + 24.5 O2(g) -> 19CO2(g) + 17H2O(l)
    (P=1 bar, T=298.15K, heat change = -1945.2 kJ)

    1. Compute percent C16H34 that reacted to form CO(g) in the process.
    2. If experiment carried out at constant V, how much heat would have been released?

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    Solution Preview

    To do this question, you need to calculate the enthalpy change for 50 g C16H34 burning by both reactions.

    Find each by using the deltaH (dH) tables provided to you in your textbook and use

    dHrxn = [Sum(products)] - ...

    Solution Summary

    This solution computes percent C16H34 and the amount of heat that would have been released.