The oxidation of copper(I) oxide, Cu2O(s), to copper(II) oxide,CuO(s), is an exothermic process.
2Cu2O + O2 = 4CuO
The change in enthalpy upon reaction of 85.49 g of Cu2O(s) is-87.23 kJ. Calculate the work, w, and energy change, ΔUrxn, when85.49 g of Cu2O(s) is oxidized at a constant pressure of 1.00 barand a constant temperature of 25 °C.
Answer in Kg.
Start by converting the mass of Cu2O that reacts (85.49 g) tothe number of moles of O2 gas consumed in the reaction. Then usethe ideal gas law to determine the change in volume (ΔV) duringthis reaction process, where Δngas is the actual amount of gasconsumed. Values for R can be found at this link.
