Heat of reaction = heat of formation of products - heat of formation of reactant

Question

Heat of reaction = heat of formation of products - heat of formation of reactants

heat of formation of CO2(g) = 393.509 kJ/mol

heat of fromation of CO(g) = -110.525 kJ/mol

heat of formation of Cu(s) = 0

heat of reaction = -393.509 kJ/mol x 1 mol - { -110.525 kJ/mol x 1 mol + 1 mol x -155 kJ/mol } = -127.984 kJ

heat released = -127.984 kJ

heat asorbed to raise the temperature from 25 oC to 1084.5 oC(q1) = nCpT

n = moles of sample = 1 basis taken

Cp = heat capacity

T = change in temperature

q1 = 1 mol x 24.5 J/mol.oC x(1084.5 - 25) oC = 25957.75 J = 25.957 kJ

now we want Cu in melted condition

heat of fusion should be added = nHfus = 1 mol x 13.0 kJ/mol = 13 kJ

enthalpy change = heat abosrbed - heat released = 25.957 kJ + 13 kJ -127.984 kJ = -89 kJ

Ans = -89 kJ

Explanation / Answer

Required HW The smelting of copper occurs by the balanced chemical equation: CuO(s) + CO(g)- Cu(s)-CO2(g) 16.1167 out of 19 12/28/17 e155 kJ/mol,Assume the process of recycling copper is simplified to just the melting of the solid point of Cu is 10845°C with Hen-130 kJ/mol and a molar heat capacity, caca-24.5 J/mol·°C. Cu starting at 25'C. The melting 3rd attempt Part 1 (0.5 point) d See Periodic Table See Hint Enthalpy change for the reaction recovering Cu from Cu

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