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: $$ 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.

Answer 1

The energy required to recycle 1.02 mol of copper involves heating it to its melting point using its molar heat capacity and then adding the phase change energy at the melting point using the enthalpy of fusion.

Step-by-step explanation:

The energy associated with the process of recycling 1.02 mol of copper involves first calculating the energy required to heat copper from room temperature (25°C) to its melting point (1084.5°C) using the specific heat capacity (cp,Cu), and then the energy for the phase change at the melting point using the enthalpy of fusion (δH°fus). The total energy (ΔE) for heating can be calculated using the formula ΔE = n × cp,Cu × ΔT, where n is the number of moles of copper, cp,Cu is the molar heat capacity, and ΔT is the temperature change. The energy for the phase change is n × δH°fus. Thus, for 1.02 moles of copper, the total energy required is ΔEtotal = (1.02 mol × 24.5 J/mol·°C × (1084.5°C - 25°C)) + (1.02 mol × 13.0 kJ/mol).