Problem: The oxidation of copper(I) oxide, Cu2O(s), to copper(II) oxide, CuO(s), is an exothermic process, 2 Cu2O(s) + O2(g) → 4 CuO (s). The change in enthalpy upon reaction of 67.68 g of Cu2O(s) is -69.06 kJ.Calculate the work, w, and the energy change, ΔUrxn, when 67.68 g of Cu2O (s) is oxidized at constant pressure of 1.00 bar and a constant temperature of 25 degree Celcius?

FREE Expert Solution

Given reaction: 2 Cu2O(s) + O2(g) → 4 CuO(s)

Given: mass of Cu2O(s) = 67.68 g Cu2O(s)

ΔHrxn = – 69.06 kJ


Calculating the mass of O2(g) that reacts with Cu2O(s):

67.68 g Cu2O×1 mol Cu2O143.1 g Cu2O×1 mol O22 mol Cu2O = 0.2365 mol O2

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Problem Details

The oxidation of copper(I) oxide, Cu2O(s), to copper(II) oxide, CuO(s), is an exothermic process, 2 Cu2O(s) + O2(g) → 4 CuO (s). The change in enthalpy upon reaction of 67.68 g of Cu2O(s) is -69.06 kJ.


Calculate the work, w, and the energy change, ΔUrxn, when 67.68 g of Cu2O (s) is oxidized at constant pressure of 1.00 bar and a constant temperature of 25 degree Celcius?

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