**Given reaction:** 2 Cu_{2}O(s) + O_{2}(g) → 4 CuO(s)

**Given:** mass of Cu_{2}O(s) = 67.68 g Cu_{2}O(s)

ΔH_{rxn} = – 69.06 kJ

**Calculating the mass of O _{2}(g) that reacts with Cu2O(s):**

$\mathbf{67}\mathbf{.}\mathbf{68}\mathbf{}\overline{)\mathbf{g}\mathbf{}{\mathbf{Cu}}_{\mathbf{2}}\mathbf{O}}\mathbf{\times}\frac{\mathbf{1}\mathbf{}\overline{)\mathbf{mol}\mathbf{}{\mathbf{Cu}}_{\mathbf{2}}\mathbf{O}}}{\mathbf{143}\mathbf{.}\mathbf{1}\mathbf{}\overline{)\mathbf{g}\mathbf{}{\mathbf{Cu}}_{\mathbf{2}}\mathbf{O}}}\mathbf{\times}\frac{\mathbf{1}\mathbf{}\mathbf{mol}\mathbf{}{\mathbf{O}}_{\mathbf{2}}}{\mathbf{2}\mathbf{}\overline{)\mathbf{mol}\mathbf{}{\mathbf{Cu}}_{\mathbf{2}}\mathbf{O}}}$ **= 0.2365 mol O _{2}**

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

Calculate the work, w, and the energy change, ΔU_{rxn}, when 67.68 g of Cu_{2}O (s) is oxidized at constant pressure of 1.00 bar and a constant temperature of 25 degree Celcius?

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Thermochemical Equation concept. You can view video lessons to learn Thermochemical Equation. Or if you need more Thermochemical Equation practice, you can also practice Thermochemical Equation practice problems.