Electrochemistry_II

What is Standard cell potential of a galvanic cell for the following reaction:

$$Fe\ \left(s\right)\ +\ Ni^{2+}\left(aq\right)\ \rightarrow\ Fe^{2+}\left(aq\right)\ +\ Ni\ \left(s\right)$$

$$E\degree_{\frac{Fe^{2+}}{Fe}}\ =\ -0.44\ V$$

$$E\degree_{\frac{Ni^{2+}}{Ni}}=-0.28\ V$$

What is the equilibrium constant at $$25\degree C$$ for the following reaction if $$E\degree_{cell}$$ is +0.16 V.

Fe (s) + Ni²⁺(aq) $$\rightarrow$$ Fe²⁺ (aq) + Ni (s)

Given: $$nFE\degree_{cell}=RT\ \ \ln K$$

R = 8.314 J/mol.K

What is E in this equation? ​ (a)  

What is $$E\degree$$ in this equation? ​ (b)  

What is n? ​ (c)  

What is Q? ​ (d)  

$$\Delta G\degree\ =-nFE\degree,\ what\ is\ the\ sign\ of\ E\degree\ for\ the\ cell\ reaction\ to\ be\ spontaeous?\ _{ }$$ ​ (a)  

What is the sign of $$\Delta G\degree$$ for the cell reaction to be spontaneous? ​ (b)  

The $$E\degree$$ of a concentration cell is always equals to ​ (c)  

The E of a concentration cell depends on the ​ (d)   of the solution in the two half cells at the given conditions.

Given a cell reaction:

$$Zn\ \left(s\right)\ +\ Cu^{2+}\left(aq\right)\ \rightarrow\ Zn^{2+}\left(aq\right)\ +\ Cu\ \left(s\right)$$

What is the correct expression for Q?

What is the nonstandard cell potential for the following reaction:

$$Cu\left(s\right)\ +2\ Ag^+\left(aq\right)\rightarrow\ Cu^{2+}\left(aq\right)\ +\ 2Ag\left(s\right)$$

Given: $$E\degree_{\frac{Ag^+}{Ag}}=0.80\ V\ \ \ \ \ \ \ \ \ \ \ \ \ E\degree_{\frac{Cu^{2+}}{Cu}}\ \ =+0.34\ V$$

[Ag⁺] = 0.25 M and [Cu²⁺] = 0.75 M