What quantity, in moles, of hydrogen is consumed in the reaction below when 307.6 kJ of energy is evolved from the combustion of a mixture of hydrogen gas and oxygen gas? H₂(g) + $\frac { 1 } { 2 }$ O₂(g) ? H₂O(l); ?_rH° = -285.8 kJ/mol-rxn

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Quizplus · Accepted Answer

The enthalpy change of the reaction is -285.8 kJ/mol-rxn. This means that for every mole of hydrogen consumed, 285.8 kJ of energy is released. Therefore, the number of moles of hydrogen consumed can be calculated as follows:```moles of hydrogen = (307.6 kJ) / (285.8 kJ/mol-rxn) = 1.076 mol```

What Quantity, in Moles, of Hydrogen Is Consumed in the Reaction