For the half-cell reaction,
`Au^(3+) + 3e^(-) rarr Au`
the value of n used in Nernest equation is:

Given , for Sn^(+4) // Sn^(2+) , standard reduction potential is 0.15 V and for Au^(3+)//Au , standard reduction potential is 1.5 V. For the reaction , 3Sn^(2+) + 2 Au^(3+) to 3 Sn^(4+) + 2 Au , the value of E_("cell")^(@) is ,

Formulate a cell from the following electrode reactions: Au^(3o+) (aq) + 3e^(Theta)rarr Au(s) Mg(s)rarr Mg^(2o+) (aq) + 2e^(Theta) .

Suppose that gold is being plated onto another metal in a electrolytic cell. The half - cell reaction producing the Au(s) is AuCl_(4)^(c-) rarr Au(s)+4Cl^(c-)+3e^(-) If a 0.30- A current runs for 15 mi n , what mass of Au(s) will be plated, assuming all the electrons are used in the reduction of AuCl_(4)?

Suppose that gold is being plated onto another metal in a electrolytic cell. The half - cell reaction producing the Au(s) is AuCl_(4)^(c-) rarr Au(s)+4Cl^(c-)+3e^(-) If a 0.30- A current runs for 1.50 mi n , what mass of Au(s) will be plated, assuming all the electrons are used in the reduction of AuCl_(4)?

Suppose that gold is being plated onto another metal in a electrolytic cell. The half - cell reaction producing the Au(s) is AuCl_(4)^(c-) rarr Au(s)+4Cl^(c-)+3e^(-) If a 0.30- A current runs for 1.50 mi n , what mass of Au(s) will be plated, assuming all the electrons are used in the reduction of AuCl_(4)?

Suppose that gold is being plated onto another metal in a electrolytic cell. The half - cell reaction producing the Au(s) is AuCl_(4)^(c-) rarr Au(s)+4Cl^(c-)+3e^(-) If a 0.30- A current runs for 1.50 mi n , what mass of Au(s) will be plated, assuming all the electrons are used in the reduction of AuCl_(4)?

Suppose that gold is being plated on to another metal in an electrolytic cell. The half - cell reaction producing the Au(s) is AuCl_(4)^(-)+3e^(-)+Au(s)+4Cl^(-) . If a 0.30 A current runs for 15.00 minute, what mass of Au(s) will be plated, assume all the electrons are used in the reduction of AuCl_(4)^(-) ? the Faraday constant is 96485 C/mol and molar mass of Au is 197.

Suppose that gold is being plated on to another metal in an electrolytic cell. The half - cell reaction producing the Au(s) is AuCl_(4)^(-)+3e^(-)+Au(s)+4Cl^(-) . If a 0.30 A current runs for 15.00 minute, what mass of Au(s) will be plated, assume all the electrons are used in the reduction of AuCl_(4)^(-) ? the Faraday constant is 96485 C/mol and molar mass of Au is 197.