Question

Copper has been used for thousands of years, either as a pure metal or in alloys. it is frequently used today in the production of wires and cables. Copper can be obtained through smelting or recycling. determine the energy associated with each of these processes in order to recycle 1.02 mol cu. the smelting of copper occurs by the balanced chemical equation: cuo co->cu co2 where δh°f,cuo is = –155 kj/mol. Assume the process of recycling copper is simplified to just the melting of the solid cu starting at 25°c. the melting point of cu is 1084.5°c with δh°fus = 13.0 kj/mol and a molar heat capacity, cp,cu = 24.5 j/mol·°c.. What is the enthalpy change for the reaction recovering cu from cuo

Answer 1

The enthalpy change for the reaction where copper is recovered from copper(II) oxide is calculated by multiplying the moles of Cu (1.02 mol) by the enthalpy of formation of CuO (-155 kJ/mol), resulting in a total exothermic enthalpy change of -158.1 kJ.

Step-by-step explanation:

The question revolves around the concept of the enthalpy change for the reaction in which copper (Cu) is recovered from copper(II) oxide (CuO) using carbon monoxide (CO) to produce copper metal and carbon dioxide (CO2). To determine the enthalpy change for the reaction, we use the given standard enthalpy of formation (δHf,COO) of CuO, which is -155 kJ/mol. We are dealing with 1.02 mol of Cu, and since the reaction is a one-to-one mole ratio for CuO and Cu, we simply multiply the moles of Cu by the enthalpy of formation of CuO to find the total enthalpy change.

To calculate the enthalpy change for the smelting process:

• Multiply the moles of Cu (1.02 mol) by the enthalpy of formation of CuO.

Total enthalpy change = 1.02 mol × (-155 kJ/mol) = -158.1 kJ

The reaction is exothermic since the enthalpy change is negative, releasing 158.1 kJ of energy when 1.02 mol of copper is smelted from copper(II) oxide.