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 25°
c.
here's my line of reasoning.. but it's been marked wrong. 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+273.1 5)= -2.609 kj
energy change = -2.609kj+ - 76.83kj = -79.439kj