Question

The following equations are half reactions and reduction potentials. Ag+ (aq) + e– Ag(s) has a reduction potential of +0.80 V. Cr3+ (aq) + 3e– Cr(s) has a reduction potential of –0.74 V. Which statement best compares the substances in these half reactions? A silver ion gains electrons more easily and is a stronger oxidizing agent than a chromium(III) ion. A silver ion loses electrons more easily and is a stronger oxidizing agent than a chromium(III) ion. A silver ion gains electrons more easily and is a stronger reducing agent than a chromium(III) ion. A silver ion loses electrons more easily and is a stronger reducing agent than a chromium(III) ion.

the answer is A

Answer 1

Answer: A

Step-by-step explanation:

Answer 2

Answer : The correct option is, (A) silver ion gains electrons more easily and is a stronger oxidizing agent than a chromium(III) ion.

Explanation :

The given half reaction are :

1st half reaction :
`Ag^+(aq)+e^-\rightarrow Ag(s)`

The reduction potential of this reaction = +0.80 V

2nd half reaction :
`Cr^(3)+(aq)+3e^-\rightarrow Cr(s)`

The reduction potential of this reaction = -0.74 V

From the reduction potentials, we conclude that the reaction which have positive reduction potential, they will gain electrons more easily and reduced itself and act as a stronger oxidizing agent.

Or we can say that the reaction which have negative reduction potential, they will lose electrons more easily and oxidized itself and act as a stronger reducing agent.

The reduction potential of 1st half reaction is positive and 2nd half reaction is negative.

Therefore, the silver ion gains electrons more easily and is a stronger oxidizing agent than a chromium(III) ion.