Unit 3 Redox

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a. 4 b. 3 c. 2 d. 1 Cr 2 O 7 2- (aq) + 14H + + 6e2Cr 3+ (aq) + 7H 2 O (l) I 2 (aq) + 2e - 2I - (aq) How many moles of I 2 are reduced by 1 mole of Cr 2 O 7 2- ions?

1 st hint The number of electrons on both sides of the redox equation must balance. a hint!!!! 2 nd hint How many more moles of Iodine are now needed?

Ans: b. 3 How many moles of I 2 are reduced by 1 mole of Cr 2 O 7 2- ions? Correct because….. The number of electrons lost and gained must be equal. Cr 2 O 7 2- (aq) + 14H + + 6e2Cr 3+ (aq) + 7H 2 O (l) I 2 (aq) + 2e - 2I - (aq) X 3 Cr 2 O 7 2- (aq) + 14H + (aq) + 3I 2 (aq)2Cr 3+ (aq) + 7H 2 O (l) + 6I - (aq)

Which of the following is not a redox reaction. a. Mg (s) + 2HCl (aq) MgCl 2 (aq) + H 2 (g) b. CuCO 3 (s) + H 2 SO 4 (aq) CuSO 4 (aq) + CO 2 (g) + H 2 O (l) c. Zn(NO 3 ) 2 (aq) + 2Ag 2AgNO 3 (aq) + 2Zn (s) d. H 2 (g) + Cl 2 (g) HCl (g)

Which reaction does not involve the formation of ions.? a hint!!!!

Which of the following is not a redox reaction. Correct because…… A redox reaction involves the transfer of electrons between reactants. a. Mg (s) + 2HCl (aq) MgCl 2 (aq) + H 2 (g) Mg H +  Mg 2+ + H 2 b. CuCO 3 (s) + H 2 SO 4 (aq) CuSO 4 (aq) + CO 2 (g) + H 2 O (l) 2H + + CO 3 2-  CO 2 + H 2 O c. Zn(NO 3 ) 2 (aq) + 2Ag 2AgNO 3 (aq) + 2Zn (s) Zn Ag  2Ag + + Zn Ans: d. H 2 (g) + Cl 2 (g) HCl (g)

In order to balance this ion-equation I – to IO 3 – You need to a. b. c. d. Number H + Number of e

1 st hint Balance the oxygen by adding water. a hint!!!! 2 nd hint Balance the hydrogen by adding H + ions. 3 rd hint Balance the charges by adding electrons

In order to balance this ion-equation I – to IO 3 – Correct because……… 1 st balance the water molecules I – + 3H 2 O  IO 3 – 2 nd balance the H using H + ions. I – + 3H 2 O  IO 3 – + 6H + 3 rd balance the charges by adding electrons I – + 3H 2 O  IO 3 – + 6H + + 6e -

The balanced redox equation for the two ion-equations below is (you will need to look a you data book, page 11) a. 2Fe (s) + 3SO 4 2- (aq) 2Fe 3+ (aq) + 3SO 3 2- (aq) b. 2Fe (s) + 3SO 4 2- (aq) + 6H + (aq) 2Fe 3+ (aq) + 3SO 3 2- (aq) + 3H 2 (g) c. 2Fe (s) + 3SO 4 2- (aq) + 6H + (aq) 2Fe 3+ (aq) + 3SO 3 2- (aq) + 3H 2 O (l) d. 3Fe (s) + SO 4 2- (aq) + 6H + (aq) Fe 3+ (aq) + SO 3 2- (aq) + 3H 2 O (l) SO 4 2- (aq) SO 3 2- (aq) Fe (s) Fe 3+ (aq)

a hint!!!! 1 st hint SO 4 2- (aq) + 2H + (aq) + 2e - SO 3 2- (aq) + H 2 O (l) 2 nd hint Fe (s) Fe 3+ (aq) + 3e -

The balanced redox equation for the two ion-equations below is (you will need to look a you data book, page 11) SO 4 2- (aq) SO 3 2- (aq) Fe (s) Fe 3+ (aq) SO 4 2- (aq) + 2H + (aq) + 2e - SO 3 2- (aq) + H 2 O (l) Correct because…… Fe (s) Fe 3+ (aq) + 3e - X 2 3SO 4 2- (aq) + 6H + (aq) + 2Fe (s) 3SO 3 2- (aq) + 3H 2 O (l) + 2Fe 3+ (aq) X 3 Ans: C

What colour change takes place during this reaction? a. Blue to colourless b. Colourless to purple c. Colourless to blue d. Purple to colourless 5 Fe 2+ (aq) + 8H + (aq) + MnO 4 - (aq)  5 Fe 3+ (aq) + Mn 2+ (aq) + 4H 2 O(l)

a hint!!!! The permanganate ion is purple.

What colour change takes place during this reaction? Correct because……….. The MnO 4 - (aq) ion is purple, while the Mn 2+ (aq) ion is colourless. 5 Fe 2+ (aq) + 8H + (aq) + MnO 4 - (aq)  5 Fe 3+ (aq) + Mn 2+ (aq) + 4H 2 O(l)

25 cm 3 of mol –1 potassium permanganate was titrated against a solution of Fe 2+ ions. The concentration of Fe 2+ ions was? 5 Fe 2+ (aq) + 8H + (aq) + MnO 4 - (aq)  5 Fe 3+ (aq) + Mn 2+ (aq) + 4H 2 O(l) Titration results, 20.5 cm 3, 20.1 cm 3 and 20.0 cm 3 a mol 1- b mol 1- c mol 1- d mol 1-

Have you used concordant titration results? a hint!!!!

n = V x C and a 5:1 ratio of mol of Fe 2+ to MnO 4 - a hint!!!!

V x x C x n x = V y x C y n y

25 cm 3 of mol –1 potassium permanganate was titrated against a solution of Fe 2+ ions. The concentration of Fe 2+ ions was? 5 Fe 2+ (aq) + 8H + (aq) + MnO 4 - (aq)  5 Fe 3+ (aq) + Mn 2+ (aq) + 4H 2 O(l) Titration results, 20.5 cm 3, 20.1 cm 3 and 20.0 cm 3 V x x C x n x = V y x C y n y X = MnO 4 - Y = Fe 3+ ( )/2 + Y 25 x = Ans : b mol 1-

The production of Aluminium during the electrolysis of aluminium oxide can be represented by a. 96,500 C b C c. 57,900 C d. 193,000 What is the quantity of electricity needed to produce 0.2 mol of Al? Al e Al

1 st hint How many moles of electrons are needed to deposit 1 mol of Al? a hint!!!! 2 nd hint The charge on a mole of electrons is 96,500C?

The production of Aluminium during the electrolysis of aluminium oxide can be represented by What is the quantity of electricity needed to produce 0.2 mol of Al? Correct because…….. To produce 1 mole of aluminium, 3 moles of electrons are needed. i.e. 96,500 C x 3 = C needed. Al e Al 1 mole Al = C 0.2 mole Al = x 0.2 = 57,900C

A solution of HCl is electrolysed. What current is needed to produce 4.8 l of H 2 gas in 3 min 13 sec? 1 mole of gas occupies 24 l. a. 20 A b. 50 A c. 100 A d. 200 A

1 st hint How many moles of hydrogen does 4.8 l represent? a hint!!!! 2 nd hint How many moles of electrons do you need to deposit 1 mol of hydrogen gas? Q = I x t

A solution of HCl is electrolysed. What current is needed to produce 4.8 l of H 2 gas in 3 min 13 sec? 1 mole of gas occupies 24 l ? Correct because…….. 2H + (aq) + 2e -  H 2 (g) So to produce a mole of hydrogen gas, 2 mol of electrons are needed. 4.8l = 4.8/24 mol = 0.2 mol of gas produced. 1 mol of gas would need x 2 C 0.2 mol would need (96500 x 2) x 0.2 C = 3860 C Quantity of charge = current x time Q = I x t So I = Q/t = 3860 / 193 = 20 A