Question

The oxidation potentials of \(A\) and \(B\) are \[ +2.37\ \mathrm{V} \quad \text{and} \quad +1.66\ \mathrm{V} \] respectively. In chemical reactions

• A. \(A\) will be replaced by \(B\)
• B. \(A\) will replace \(B\)
• C. \(A\) will not replace \(B\)
• D. \(A\) and \(B\) will not replace each other

Hint:

Higher oxidation potential: \[ \Rightarrow \] greater tendency to lose electrons \[ \Rightarrow \] stronger reducing agent.

Answer 1

The Correct Option is B

Step 1: Understand oxidation potential.
Greater oxidation potential means greater tendency to: \[ \text{lose electrons} \] Hence stronger reducing agent. Given: \[ E^\circ_{\mathrm{ox}}(A)=+2.37\ \mathrm{V} \] \[ E^\circ_{\mathrm{ox}}(B)=+1.66\ \mathrm{V} \] Thus: \[ A \] has greater tendency to oxidize than: \[ B \]

Step 2: Determine displacement tendency.
A stronger reducing agent displaces a weaker reducing agent from its salt solution. Since: \[ A>B \] in oxidation tendency, \[ A \] will replace: \[ B \]

Step 3: Identify the correct option.
Therefore: \[ \boxed{ \mathrm{(B)\ A\ will\ replace\ B } } \]