The oxidation of copper(I) oxide, Cu2O(s), to copper(II) oxide, CuO(s), is an exothermic process. 2Cu2O(s)+O2(g)⟶4CuO(s)ΔH∘rxn=−292.0 kJmol...

Question

Question

The oxidation of copper(I) oxide, Cu2O(s), to copper(II) oxide, CuO(s), is an exothermic process.

2Cu2O(s)+O2(g)⟶4CuO(s)ΔH∘rxn=−292.0 kJmol

Calculate the energy released as heat when 62.29 g Cu2O(s) undergo oxidation at constant pressure.

energy released: kJ

Answer 1

Answer #1

The enthalpy of the reaction = −292.0 kJ/mol

According to the balanced reaction, when two mole of Cu2O is oxidized that will release 292 kJ of heat

Mass of Cu2O used = 62.29 g

Molar mass of Cu2O = 143.09 g/mol

Moles of Cu2O used = 62.29 g/143.09 g/mol = 0.4353 Moles

The amount heat released for 0.4353 moles of Cu2O = −292.0 kJ x 0.4353 mol / 2 mol = 63.5538 kJ

Hence 63.5538 kJ of energy will be released when 62.29 g Cu2O(s) undergo oxidation at constant pressure

Answer 2

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