I tried and it says I'm wrong. I am very frustrated please help.There is also a second part I need help with. Problem is asfollows:
Write a balanced net ionic equation for the redox reaction of Ag2S and Al metal that produces Ag metal and AI(OH)3. Be sure to include phases for each species in the equation. 3Ag2 S(s) + 2Al(s) + 6 OH- (aq) rightarrow 3Ag(s) + 3S2- (aq) + 2Al (OH) 3(s) Tip: Plus signs (+) can be typed from the keyboard. Reaction arrows can be found in the Tools menu of the answer module. Include phases in the balanced chemical equation. Click on the (aq) button in the tools to select the phase to add. Phases should not be subscripted. Calculate E degree for the reaction in Part a. [Hint: Derive E degree values for the half-reactions in which Ag2S is reduced to Ag metal and Al(OH)3 is reduced to Al metal. You can do this by combining the standard potentials for the reduction of Ag+ and Al3+ in Appendix 6 with the Ksp expressions and values of Ag2S (Ksp = 1.6 times 10-49) and AI(OH)3 (Ksp = 1.9 times 10-33).
