The standard electrode potential for the half-cell containing Fe 2 + aq and Fe 3 + aq is + 0 . 77 V . Use the relationship E = E ° + 0 . 059 z log oxidised form reduced form to calculate the electrode potential at 298 K if the concentration of Fe 2 + aq is 0 . 02 mol dm - 3 and the concentration of Fe 3 + aq is 0 . 1 mol dm - 3 .

Given, E ∘ Fe 3 + / Fe 2 + = + 0 . 77 V , Fe 2 + = 0 . 02 mol dm - 3 and Fe 3 + = 0 . 1 mol dm - 3 . E = E ° + 0 . 059 z log oxidised form reduced form = 0 . 77 + 0 . 059 1 log 0 . 1 0 . 02 = 0 . 811 V Therefore, E = 0 . 811 V .

The standard electrode potential for the half-cell containing Fe 2 + aq and Fe 3 + aq is + 0 . 77 V . Use the relationship E = E ° + 0 . 059 z log oxidised form reduced form to calculate the electrode potential at 298 K if the concentration of Fe 2 + aq is 0 . 02 mol dm - 3 and the concentration of Fe 3 + aq is 0 . 1 mol dm - 3 .

Given, E ∘ Fe 3 + / Fe 2 + = + 0 . 77 V , Fe 2 + = 0 . 02 mol dm - 3 and Fe 3 + = 0 . 1 mol dm - 3 . E = E ° + 0 . 059 z log oxidised form reduced form = 0 . 77 + 0 . 059 1 log 0 . 1 0 . 02 = 0 . 811 V Therefore, E = 0 . 811 V .

The standard electrode potential for the half-cell containing Ag + aq and Ag s is + 0 . 80 V . Calculate the electrode potential at 298 K if the concentration of Ag + aq is 0 . 05 mol dm - 3 .

Given, E ∘ Ag + / Ag = + 0 . 80 V , Ag + aq = 0 . 05 mol dm - 3 , and = 298 K . We know that, E = E ° + 0 . 059 z log oxidised form reduced form = 0 . 80 + 0 . 059 1 log 0 . 05 = 0 . 723 V Therefore, E = 0 . 723 V .

EASY

AS and A Level

IMPORTANT

Earn 100

The standard electrode potential for the half-cell containing ${Fe}^{2 +} (aq)$ and ${Fe}^{3 +} (aq)$ is $+ 0.77 V$ . Use the relationship $E = E^{°} + \frac{0.059}{z} \log \frac{[oxidised form]}{[reduced form]}$ to calculate the electrode potential at $298 K$ if the concentration of ${Fe}^{2 +} (aq)$ is $0.02 mol {dm}^{- 3}$ and the concentration of ${Fe}^{3 +} (aq)$ is $0.1 mol {dm}^{- 3}$ .

Important Questions on Electrochemistry

EASY

AS and A Level

IMPORTANT

Chemistry for Cambridge International AS & A Level Coursebook with Digital Access (2 Years)>Chapter 20 - Electrochemistry>EXAM-STYLE QUESTIONS>Q 9

The standard electrode potential for the half-cell containing

{Fe}^{2 +} (aq)

and

{Fe}^{3 +} (aq)

+ 0.77 V

. Using the relationship

E = E^{°} + \frac{0.059}{z} \log \frac{[oxidised form]}{[reduced form]}

explain why the standard electrode potential for the half-cell containing

{Fe}^{2 +} (aq)

and

{Fe}^{3 +} (aq)

is always

+ 0.77 V

if there are equimolar concentrations of

{Fe}^{2 +} (aq)

and

{Fe}^{3 +} (aq)

EASY

AS and A Level

IMPORTANT

Chemistry for Cambridge International AS & A Level Coursebook with Digital Access (2 Years)>Chapter 20 - Electrochemistry>EXAM-STYLE QUESTIONS>Q 9

The standard electrode potential for the half-cell containing

{Ag}^{+} (aq)

and

Ag (s)

+ 0.80 V

. Calculate the electrode potential at

298 K

if the concentration of

{Ag}^{+} (aq)

0.05 mol {dm}^{- 3}

EASY

AS and A Level

IMPORTANT

Chemistry for Cambridge International AS & A Level Coursebook with Digital Access (2 Years)>Chapter 20 - Electrochemistry>EXAM-STYLE QUESTIONS>Q 9

Predict whether the reaction ${Fe}^{2 +} (aq) + {Ag}^{+} (aq) \overset{}{⇌} {Fe}^{3 +} (aq) + Ag (s)$ is likely to occur at the concentrations ${Fe}^{2 +} (aq) 0.05 mol {dm}^{- 3}$ , ${Fe}^{3 +} (aq) 0.1 mol {dm}^{- 3}$ and ${Ag}^{+} (aq) 0.05 mol {dm}^{- 3}$ . Explain your answer.

Given, ${E^{\circ}}_{{Ag}^{+} / Ag} = + 0.80 V$ and ${E^{\circ}}_{{Fe}^{3 +} / {Fe}^{2 +}} = + 0.77 V$ .

EASY

AS and A Level

IMPORTANT

Chemistry for Cambridge International AS & A Level Coursebook with Digital Access (2 Years)>Chapter 20 - Electrochemistry>EXAM-STYLE QUESTIONS>Q 10

Concentrated aqueous sodium chloride can be electrolysed in the laboratory using graphite electrodes. Write the formulae for all the ions present in an aqueous solution of sodium chloride.

EASY

AS and A Level

IMPORTANT

Chemistry for Cambridge International AS & A Level Coursebook with Digital Access (2 Years)>Chapter 20 - Electrochemistry>EXAM-STYLE QUESTIONS>Q 10

Concentrated aqueous sodium chloride can be electrolysed in the laboratory using graphite electrodes. Write half-equations to show the reaction at the anode.

EASY

AS and A Level

IMPORTANT

Chemistry for Cambridge International AS & A Level Coursebook with Digital Access (2 Years)>Chapter 20 - Electrochemistry>EXAM-STYLE QUESTIONS>Q 10

Concentrated aqueous sodium chloride can be electrolysed in the laboratory using graphite electrodes. Write half-equations to show the reaction at the cathode.

EASY

AS and A Level

IMPORTANT

Chemistry for Cambridge International AS & A Level Coursebook with Digital Access (2 Years)>Chapter 20 - Electrochemistry>EXAM-STYLE QUESTIONS>Q 10

Concentrated aqueous sodium chloride can be electrolysed in the laboratory using graphite electrodes. Explain why the reaction at the anode is classed as oxidation.

EASY

AS and A Level

IMPORTANT

Chemistry for Cambridge International AS & A Level Coursebook with Digital Access (2 Years)>Chapter 20 - Electrochemistry>EXAM-STYLE QUESTIONS>Q 10

Concentrated aqueous sodium chloride can be electrolysed in the laboratory using graphite electrodes. After a while, the solution near the cathode becomes very alkaline. Explain why?

The standard electrode potential for the half-cell containing Fe2+aq and Fe3+aq is +0.77 V. Use the relationship E=E°+0.059zlogoxidised formreduced form to calculate the electrode potential at 298 K if the concentration of Fe2+aq is 0.02 mol dm-3 and the concentration of Fe3+aq is 0.1 mol dm-3.

Important Questions on Electrochemistry

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