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18 Nov 2019
1. What should be the activity of zinc sulfate (ZnSO4) for the following reaction to be (a) at equilibrium, (b) to take place from left to right, (c) to take place from right to left in a solution of ZnSO4 and sulfuric acid (H2SO,) at pH-4 and at 1 atm and 25°C. Zn + H2SO4 = ZnSO4 + H2 2. Assuming standard states and using the half cell reaction [Ag(CN)2 + e-=Ag + 2CN, eo-0.31 V. e the spontaneous direction of the following reaction by calculating the cell potential. 2Ag + 2H,0 + 4KCN = 2AgK(CN)2 +H2 +2KOH 3. Write all possible electrochemical half-cell reactions for oxidation (anodic) and reduction (cathodic) during uniform corrosion of iron (Fe) - cupper (Cu) alloy in an aerated solution of zinc sulfate (ZnSO4), stannic chloride (SnCl4), and sulfuric acid (H2SO4). [Hint: Cu is stable in neutral form and charged Fe, Zn and Sn are stable in Fe2*, Zn2 and Sn2* forms, respectively.]
1. What should be the activity of zinc sulfate (ZnSO4) for the following reaction to be (a) at equilibrium, (b) to take place from left to right, (c) to take place from right to left in a solution of ZnSO4 and sulfuric acid (H2SO,) at pH-4 and at 1 atm and 25°C. Zn + H2SO4 = ZnSO4 + H2 2. Assuming standard states and using the half cell reaction [Ag(CN)2 + e-=Ag + 2CN, eo-0.31 V. e the spontaneous direction of the following reaction by calculating the cell potential. 2Ag + 2H,0 + 4KCN = 2AgK(CN)2 +H2 +2KOH 3. Write all possible electrochemical half-cell reactions for oxidation (anodic) and reduction (cathodic) during uniform corrosion of iron (Fe) - cupper (Cu) alloy in an aerated solution of zinc sulfate (ZnSO4), stannic chloride (SnCl4), and sulfuric acid (H2SO4). [Hint: Cu is stable in neutral form and charged Fe, Zn and Sn are stable in Fe2*, Zn2 and Sn2* forms, respectively.]
Reid WolffLv2
24 Apr 2019