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
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.
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.
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 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.
What is the difficulty of this problem?
Our tutors rated the difficulty ofThe oxidation of copper (l) oxide, Cu 2O(s), to copper(II) o...as medium difficulty.
How long does this problem take to solve?
Our expert Chemistry tutor, Dasha took 4 minutes and 9 seconds to solve this problem. You can follow their steps in the video explanation above.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Hascall's class at NAU.