The activity coefficient of copper in iron at infinite dilution, relative to pure copper as the standard state, is 8.5 at 1600°C (1873 K). Calculate the free energy change for the reaction {Cu> = CHe.wtil at 1600°C (1873 K). Assume the atomic weights of copper and iron to be 63.5 and 55.85 respectively.

The melting point of cobalt is 1480°C (1753 K). Calculate the free energy change for the transfer of one g-atom of cobalt from pure liquid to a 1 wt % solution in liquid iron at 1500°C (1773 K). Assume that cobalt behaves ideally in iron at that temperature. Atomic weights of Co and Fe are 58.9 and 55.85 respectively.

The vapour pressure of copper over Cu-Fe alloys at 1550°C (1823 K), as a function of composition, is given below. xCu PCu (mm Hg) ; (pCu(N/m2) : 1.0 0.547 72.93 0.792 0.486 64.79 0.476 0.449 59.86 0.217 0.399 53.20 ) Calculate the activity of iron at x~ = 0.217, assuming that the alpha-func­ tion istthlesame forboth iron andcopper atthis concentration at1550°C (1823 K).

2Cu+ (aq) → Cu (s) + Cu+ (aq) 2Cu+ (𝑎𝑞) → Cu (𝑠) + Cu+ (𝑎𝑞) is +0.36 V at 298 K. The equilibrium constant of the reaction is

The excess partial molar free energy of zinc in liquid Cu-Zn alloys at 1027°C (1300 K) can be represented as 2 G^ (cal/mole) = -5150 (1 -xZn) . Calculate the activity of copper at 1027 C (1300 K) in an equiatomic solution.

The cycle of copper reactions starts with solid copper metal and ends with solid copper metal.Suppose you start with 0.500 g of Cu. After performing all the reactions, you have 0.460 g of Cu. What percentage of the copper did you recover?