Question

The information below describes a redox reaction.

Answer 1

Answer : The coefficient of silver in the final, balanced equation for this reaction is, 3

Explanation :

Redox reaction or Oxidation-reduction reaction : It is defined as the reaction in which the oxidation and reduction reaction takes place simultaneously.

Oxidation reaction : It is defined as the reaction in which a substance looses its electrons. In this, oxidation state of an element increases. Or we can say that in oxidation, the loss of electrons takes place.

Reduction reaction : It is defined as the reaction in which a substance gains electrons. In this, oxidation state of an element decreases. Or we can say that in reduction, the gain of electrons takes place.

The given redox reaction is,

$Ag^+(aq)+Al(s)\rightarrow Ag(s)+Al^{3+}(aq)$

The oxidation-reduction half reaction will be :

Oxidation : $Al\rightarrow Al^{3+}+3e^-$

Reduction : $Ag^{+}+1e^-\rightarrow Ag$

In order to balance the electrons, we multiply the reduction reaction by 3 and then added both equation, we get the balanced redox reaction.

The balanced redox reaction will be,

$3Ag^+(aq)+Al(s)\rightarrow 3Ag(s)+Al^{3+}(aq)$

From the balanced redox reaction we conclude that, the coefficient of silver in the final balanced equation for this reaction is 3.

Hence, the correct option is 3.

Answer 2

Answer:

3

Explanation:

You have to mutiply the silver reaction by 3 in order to substract the electrons