Saturday
October 25, 2014

Homework Help: Chemistry

Posted by DC on Sunday, November 3, 2013 at 8:40pm.

help - confusion :(

The oxidation of copper(I) oxide, Cu2O(s), to copper(II) oxide, CuO(s), is an exothermic process,
2 Cu2O + O2 --> 4CuO

The change in enthalpy upon reaction of 75.30 g of Cu2O(s) is -76.83 kJ. Calculate the work, w, and energy change, ΔUrxn, when 75.30 g of Cu2O(s) is oxidized at a constant pressure of 1.00 bar and a constant temperature of 25C.

Here's my line of reasoning.. but it's been marked wrong. Thank you in advance.

converting 75.3g of Cu2O to moles of CuO, I got 1.0525mol CuO

W=-delta(n)RT = -(1.0525mol)(8.3144J/molK)(25+273.15)= -2.609 kJ

energy change = -2.609kj+ - 76.83kJ = -79.439kJ

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