Hi, I am struggling with this question in my homework

Hi, I am struggling with this question in my homework. I need to understand the method needed to get the correct answer.Consider the following reactions:Zn2+ + 4NH3 ā†’ Zn(NH3)4 Ī²= 5.01 x 10^8Zn2+ + 2e- ā†’ Zn(s) Eāˆ˜ = -0.762Assuming there is negligible current and nearly all Zn2+ is in the form Zn(NH3)4 , what cathode potential (vs. S.H.E.) would be required to reduce 99.99% of the Zn2+ from a solution containing 0.13M Zn2+ in 1.0 M ammonia(NH3)? (Assume T = 298 K).

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