# Problem: The oxidation of copper(I) oxide, Cu 2O(s), to copper(II) oxide, CuO(s), is an exothermic process.2CuO2(s) + O2(g) → 4CuO(s)The change in enthalpy upon reaction of 67.68 g of CuO (s) is -69.06 kJCalculate the work, w, and the energy change, ΔU rxn, when 67.68 g of Cu 2O (s) is oxidized at constant pressure of 1.00 bar and at constant temperature of 25°C?

###### FREE Expert Solution

We’re being asked to calculate the work, w, and the energy change, ΔU rxn when 67.68 g of CuO2 (s) is oxidized at constant pressure of 1.00 bar and at constant temperature of 25°C

The given reaction is:

2CuO2(s) + O2(g) → 4CuO(s)

* always check if it is balanced

Recall that work (w) is given by:

$\overline{){\mathbf{w}}{\mathbf{=}}{\mathbf{-}}{\mathbf{P\Delta V}}}$

where:

P = pressure (in atm)

ΔV = Vfinal – Vinitial = change in volume (in L)

Also note that if work is:

• (+): work is done by the surroundings to the system (compression)

• (–): work is done by the system to the surroundings (expansion)

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###### Problem Details

The oxidation of copper(I) oxide, Cu 2O(s), to copper(II) oxide, CuO(s), is an exothermic process.

2CuO2(s) + O2(g) → 4CuO(s)

The change in enthalpy upon reaction of 67.68 g of CuO (s) is -69.06 kJ

Calculate the work, w, and the energy change, ΔU rxn, when 67.68 g of Cu 2O (s) is oxidized at constant pressure of 1.00 bar and at constant temperature of 25°C?