Which of the following chemical equations show(s) oxidation-reduction reactions? 1. mg(s) + i2(aq) --> mgi2(s)2. pb(clo4)2(aq) + 2 ki(aq) --> pbi2(s) + 2 kclo4(aq)3. fe2o3(s) + 3 co(g) --> 2 fe(s) + 3 co2(g)1 only2 only1 and 21 and 32 and 3

Answer : The correct option is, 1 and 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.

(1) The given balanced chemical reaction is :

The oxidation-reduction half reaction will be :

Oxidation :

Reduction :

In this reaction, the oxidation state of 'Mg' changes from (0) to (+2) that means Mg lost 2 electrons and it shows oxidation and the oxidation state of 'I' changes from (0) to (-2) that means 'I' gains 2 electrons and it shows reduction.

(2) The given balanced chemical reaction is :

In this reaction does not shows oxidation reduction reaction. This reaction shows double displacements and in this reaction the oxidation state of lead, iodine, potassium and chlorate does not change.

(3) The given balanced chemical reaction is :

The oxidation-reduction half reaction will be :

Oxidation :

Reduction :

In this reaction, the oxidation state of 'C' changes from (+2) to (+4) that means C lost 2 electrons and it shows oxidation and the oxidation state of 'Fe' changes from (+3) to (0) that means 'Fe' gains 3 electrons and it shows reduction.

Hence, the chemical equations show(s) oxidation-reduction reactions are, 1 and 3.

1.consider the following balanced equation and answer parts a through. show calculations for each part.  

3 ag(s) + 4 hno3(aq) → 3 agno3(aq) + no(g) + 2 h2o(l)  

a. calculate the number of moles of agno3 produced by the reaction of 3 moles of ag with excess hno3. if the number to the left of the compound represents the number of moles of the compound which are present, then 3 moles of ag react with 4 moles hno3 to produce 3 moles agno3 (aq).

so the answer to a would be 3 moles.

b. calculate the number of moles of agno3 produced by the reaction of 108 grams of ag with excess hno3.  

i'm not sure how to plug in the grams of silver into an equation using moles to find how many moles are produced.

c. calculate the number of grams of agno3 produced by the reaction of 108 grams of ag with excess hno3  

d. calculate the number of moles of no produced as a byproduct of the reaction of 108 grams of ag with excess hno3.  

e. calculate the number of grams of no produced as a byproduct starting with 108 grams of ag and excess hno3.  

explanation: