Question

Question #b15c6

Answer 1

This requires the Nernst equation,

`E = E^° - (0.0592)/n * logQ`

We have an equilibrium here,

`2Cr(s) + 3Cl_2(g) to 6Cl^(-)(aq) + 2Cr^(3+)(aq)`,

where `E° = 0.618V`, and

`K = ([Cl^-]^6[Cr^(3+)]^2)/([Cl_2]^3)`

Hence,

`1.77V = 0.618V - (0.0592)/6 * log((1^6*x^2)/(1^3))`
`therefore x = [Cr^(3+)] approx 4.43*10^-26M`

This is fairly unreasonable, I agree with the Ernest and Michael.