We’re being asked to determine the heat (q) released by the reaction of 50.05 g Cu2O.
The given reaction is:
2 Cu2O(s) + O2(g) → 4 CuO(s); ΔH˚rxn = –292.0 kJ/mol
From the balanced equation, we can see that the given ΔH˚rxn (–292.0 kJ) corresponds to 2 moles of Cu2O.
Recall that at constant pressure, heat is equivalent to enthalpy.
The oxidation of copper (l) oxide, Cu 2O(s), to copper(II) oxide, CuO(s), is an exothermic process,
2Cu2O(s) + O2(g) → 4CuO(s) ΔH°rxn = -292.0 kJ/mol
Calculate the energy released as heat (kJ) when 50.05 g of Cu 2O(s) undergo oxidation at constant pressure.
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