Question

The standard electrode potentials of Zn, Ag and Cu are \(-0.76\), \(+0.80\) and \(+0.34\) V respectively. Identify the correct statement from the following.

• A. Ag can oxidize Zn and Cu
• B. Ag can reduce \(Zn^{2+}\) and \(Cu^{2+}\)
• C. Zn can reduce \(Ag^+\) and \(Cu^{2+}\)
• D. Cu can oxidize Zn and Ag

Hint:

Lower standard reduction potential means stronger reducing nature of the metal.

Answer 1

The Correct Option is C

Step 1: Given standard electrode potentials: \[ E^\circ_{Zn^{2+}/Zn}=-0.76\,V \] \[ E^\circ_{Cu^{2+}/Cu}=+0.34\,V \] \[ E^\circ_{Ag^+/Ag}=+0.80\,V \]

Step 2: A metal with lower reduction potential has greater tendency to get oxidized.

Step 3: Zinc has the lowest reduction potential, so zinc is the strongest reducing agent among the given metals.

Step 4: A reducing agent reduces other ions and itself gets oxidized.

Step 5: Therefore, zinc can reduce: \[ Ag^+ \rightarrow Ag \] and \[ Cu^{2+} \rightarrow Cu \] \[ \boxed{\text{Zn can reduce \(Ag^+\) and \(Cu^{2+}\)}} \]