Quick questions on Redox reactions and the electrochemical series: VCE Chemistry Unit 3

6short Q&A pairs drawn directly from our worked dot-point answer. For full context and worked exam questions, read the parent dot-point page.

What are redox in terms of electrons?

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A redox reaction involves the transfer of electrons between species.

What are half-equations?

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A half-equation shows just one half of the redox process (the oxidation OR the reduction), including the electrons transferred. Half-equations must be balanced for atoms and charge.

What is the electrochemical series?

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The electrochemical series (in your VCAA data book) lists half-equations written as reductions with their standard electrode potentials (E°) measured at 25°C, 1 mol L^-1 (or 1 atm for gases), against the standard hydrogen electrode (SHE = 0.00 V).

What is q1?

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Using standard electrode potentials, determine whether copper will displace silver from

\text{AgNO}_3

solution.

E^{\circ}(\text{Cu}^{2+} | \text{Cu}) = +0.34 \, \text{V}

E^{\circ}(\text{Ag}^+ | \text{Ag}) = +0.80 \, \text{V}

. [3 marks]

What is q2?

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Balance the redox equation between

\text{Cr}_2 \text{O}_7^{2-}

and

\text{Fe}^{2+}

in acidic solution. (a) Write each half-equation. (b) Add to give the overall equation.

What is q3?

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Consider a galvanic cell with

\text{Ni} | \text{Ni}^{2+}

(

E^{\circ} = -0.25 \, \text{V}

) and

\text{Ag} | \text{Ag}^+

(

E^{\circ} = +0.80 \, \text{V}

). (a) Calculate

E^{\circ}_{cell}

. (b) Write the spontaneous overall equation.

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