# Problem: The oxidation of copper (l) oxide, Cu 2O(s), to copper(II) oxide, CuO(s), is an exothermic process, 2Cu2O(s) + O2(g) → 4CuO(s)                    ΔH°rxn = -292.0 kJ/mol Calculate the energy released as heat (kJ) when 50.05 g of Cu 2O(s) undergo oxidation at constant pressure.

###### FREE Expert Solution
90% (231 ratings)
###### FREE Expert Solution

We’re being asked to determine the heat (q) released by the reaction of 50.05 g Cu2O

The given reaction is:

2 Cu2O(s) + O2(g)  4 CuO(s); ΔH˚rxn = –292.0 kJ/mol

From the balanced equation, we can see that the given ΔH˚rxn (–292.0 kJ) corresponds to 2 moles of Cu2O

Recall that at constant pressure, heat is equivalent to enthalpy.

90% (231 ratings)
###### Problem Details

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

2Cu2O(s) + O2(g) → 4CuO(s)                    ΔH°rxn = -292.0 kJ/mol

Calculate the energy released as heat (kJ) when 50.05 g of Cu 2O(s) undergo oxidation at constant pressure.

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 Equations concept. You can view video lessons to learn Thermochemical Equations. Or if you need more Thermochemical Equations practice, you can also practice Thermochemical Equations practice problems.

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Our tutors rated the difficulty ofThe oxidation of copper (l) oxide, Cu 2O(s), to copper(II) o...as medium difficulty.

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Based on our data, we think this problem is relevant for Professor Hascall's class at NAU.