Advantage zone map of Cu-S-water system

First, free energy data

The components considered for sulfur and the data used are listed in Table 1. Data containing the copper component under consideration are shown in Table 2 below.

Table 1 Free energy of each substance in the S-H 2 O system

substance

S 2 -

HS -

H 2 S(aq)

SO 4 2 -

HSO 4 -

H 2 O(1)

△G Θ ∕kJ

+111.4

+12.08

-27.83

-744.53

-755.91

-237.129

Table 2 Free energy data for the formation of various copper-containing components

substance

Cu +

Cu 2 +

CuO

Cu 2 O

CuO 2 2 -

HcuO -

Cu 2 S

CuS

△G Θ ∕kJ

49.98

65.49

-129.7

-146.0

-183.6

-258.5

-86.2

-53.6

Second, the equilibrium equation

Third, the advantage zone map and its analysis

Figure 1 is a diagram of the Cu-S-H 2 O dominant zone in the solution with a sulfur-containing activity of 0.1 mol ∕L and a copper ion activity of 10 -3 and 10 -6 mol ∕L. . The Cu-H 2 O system dominant zone map of the same activity value has a stable zone free of sulfides, and the boundary between Cu 2 + and Cu, ie, equilibrium 7, extends to the axis of pH=0. That is, CuS and Cu 2 S region are non-occurrence of the region in FIG advantage when the presence area of the metal copper sulfide stationary phase, and extends slightly Cu 2 + region. There is no Cu + stable region in the figure, so |Cu + | is less than 10 -6 mol∕L at 298.15K. The low activity ion balance produced by copper oxide and H 2 CuO 2 at pH=13 or higher.

Figure 1 Cu-S-H 2 O dominant area map

(298K, S and H 2 S activity is 10 -1 , Cu ion activity is 10 -3 or 10 -6 )

If FIG. 2 on the activity of sulfur species to elemental sulfur is 10 -1 to 1 Videos stable region, all it within the stability region of CuS. Therefore, elemental sulfur can coexist thermodynamically with CuS at 298.15 K, but does not coexist with Cu 2 S. The figure clearly indicates that under acidic oxidation conditions, the chalcopyrite Cu 2 S and copper blue CuS can theoretically be leached to produce a solution containing Cu 2 + but not containing Cu + , and the contained sulfur is oxidized to Elemental sulfur, or oxidized to sulfate at a higher potential E. The conditions required for the reaction to proceed are that the potential E value in the solution is maintained at a relatively high value so that no H 2 S or its dissociated ions are present in the solution. The boundary line between HSO 4 - and SO 4 2 - is also plotted on the graph, because the equilibrium line between Cu 2 S and Cu 2 + represented by equilibrium (k) and formula (l) changes the slope at this pH. The equilibrium line between Cu 2 S and CuS represented by the equilibrium formula (q) and the formula (r) also changes the slope, but is hardly seen on the graph.

Figure 2 S-H 2 O dominant area map

(298K, S and H 2 S activities are 10 -1 or 10 -4 respectively )

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