Question

Consider the following table of standard electrode potentials for a series of hypothetical reactions in aqueous solution: Reduction Half-Reaction A+ (aq) + e + A(8) B2+ (aq) + 2e → B(s) C18+ (aq) + e + C2+ (aq) D3+ (aq) + 3e + D(s) E° (V) 1.33 0.87 -0.12 -1.59 Part A Which substance is the strongest oxidizing agent? O D3+ (aq) O A+ (aq) O c3+ (aq) OB2+ (aq) Submit Request Answer

Answer 1

Answer:-

As we know that according to the standard reduction potential of electrode at 298 K i.e standard electrochemical series of the electrodes, the electrode potential of the electrodes which are above the hydrogen electrode (standard electrode potential) i.e electrodes having positive value of electrode potential behave as oxidizing agent which means that strong affinity to accept the electrons. The high positive value of electrode potential indicates that strong oxidizing power of the electrode. Also we know that oxidizing power of the electrode increased with decrease reducing power of the electrode i.e weak reducing agent.

So the electrode potential of the electrodes which are below the hydrogen electrode (standard electrode potential) i.e electrodes having negative value of electrode potential behave as reducing agent which means that strong tendency to donate the electrons. The high negative value of electrode potential indicates that strong reducing power of the electrode. Also we know that reducing power of the electrode increased with decrease oxidizing power of the electrode i.e weak oxidizing agent.

Since we know that

Electrodes	Electrode potential (E0) V
A+(aq) + e- $\rightarrow$ A(s)	1.33 V
B2+(aq) + 2e- $\rightarrow$ B(s)	0.87 V
C3+(aq) + e-  $\rightarrow$ C2+(aq)	- 0.12 V
D3+(aq) + 3e-  $\rightarrow$ D(s)	- 1.59 V

therefore order of oxidizing power of electrodes i.e oxidizing agent order is as follows:-

A⁺_(aq) >   B²⁺_(aq) > C³⁺_(aq) > D³⁺_(aq)

Part -A -

therefore strong oxidizing agent = A⁺_(aq)

So correct option is A⁺_(aq)

Part -B -

weak oxidizing agent =  D³⁺_(aq)

So correct option is D³⁺_(aq)

So the order of reducing power of electrodes i.e reducing agent order is as follows:-

D_(s) > C²⁺_(aq) > B_(s) > A_(s)

Part -C-

therefore strong reducing agent =  D_(s)

So correct option is D_(s)

Part -D​​​​​​​-

therefore weak reducing agent =  A_(s)

So correct option is A_(s)

Part -E​​​​​​​-

As we know that C²⁺_(aq) has negative value of electrode potential i.e -0.12 V which shows that it has strong tendency to donate electron as compared to the A_(s) and B_(s) therefore it easily oxidized the A_(s) and B_(s) whereas D³⁺_(aq) has high negative value of electrode potential i.e - 1.59 V as compared to the C²⁺_(aq) which shows that it has strong tendency to donate electron as compared to the C²⁺_(aq) therefore it can easily oxidized the C²⁺_(aq) .

So correct option is D³⁺_(aq)