1b.3 displacment reactions

Question 1

do metal displacment reaction in (aq) solutions require enegry

Answer 1

no, they dont

Question 2

do metal displacement reaction in (s) states require energy

Answer 2

yes, they do

Question 3

why are metal displacement reactions consider redox reactions?

Answer 3

because the more reactive element would give a number of electrons to the less reactive element in order to displace it making the less reactive element reduced and the more reactive element oxidized

Question 4

reaction 1: Mg(s) + CuSO4(aq) —–> Cu(s) + MgSO4(aq)
reaction 2 : 2AL(s) + Fe2O3(s) —-> 2Fe(s) + Al2O3
what do these two reaction have in similar

Answer 4

1. they both involve one metal reacting with a compound of a different metal
2. both produce metal and a different metal compound
3. both are redox reactions
4. in both cases the more reactive metal in the reactant side has taken the place of the less reactive metal in the compound

Question 5

reaction 1: Mg(s) + CuSO4(aq) —–> Cu(s) + MgSO4(aq)
reaction 2 : 2AL(s) + Fe2O3(s) —-> 2Fe(s) + Al2O3
whatis the diffrence between these two reactions

Answer 5

1. reaction 1 takes place in an (aq) solution while reaction 2 takes place in an (s) state
2. reaction 1 needs no energy to start but reaction 2 requires a lot of energy
3. reaction 1 is most likely done in a laboratory, but reaction 3 is for specific purpose in the industry

Question 6

Mg(s) + CuSO4(aq) —–> Cu(s) + MgSO4(aq) what do we observe in this reaction

Answer 6

the blue solution would turn paler and if we added more magnesium it would become colorless

Question 7

Mg(s) + CuSO4(aq) —–> Cu(s) + MgSO4(aq) what elemnt is oxidesed and what element is reduced

Answer 7

Cu ions are reduced because Mg atoms transfer two electrons to the Cu making Mg oxidized

Question 8

what is 2AL(s) + Fe2O3(s) —-> 2Fe(s) + Al2O3 used in

Answer 8

this reaction is used in joining rails together since both rails are good conductors of heat it would be very hard to join them together, so the thermite method s used where Al and FeO are placed above the 2 rails then a magnesium fuel is lit making the reaction seen in the question start. The reaction is so exothermic that the Fe formed would be in a molten form which would follow in between the two rails and cool down making them join

Question 9

2AL(s) + Fe2O3(s) —-> 2Fe(s) + Al2O3 what elemnt is oxidesed and what element is reduced

Answer 9

Al is oxidized and Fe is reduced since Al atoms transfer 3 electrons to Fe ions in order to displace it

Question 10

Cl2(aq) + KBr(aq) —> 2Br(aq) + KCl(aq) what elemnt is reduced and what element is oxidesed

Answer 10

Cl is reduced and Br is oxidized since Cl atoms take 2 electrons from Br ions in order to displace it

Question 11

why are halogen displacement reactions consider redox reactions?

Answer 11

because the more reactive halogen would take electrons from the less reactive halogen to displace it making the more reactive halogen reduced and the less reactive halogen oxidized