Consider the table of standard reduction potentials shown below.

Half-reaction $E^{\circ}$
$C l_{2} + 2 e^{-} \to 2 C l^{-}$ $1.36 V$
$O_{2} + 4 H^{+} + 4 e^{-} \to 2 H_{2} O$ $1.23 V$
$2 H_{2} O + 2 e^{-} \to H_{2} + 2 O H^{-}$ $- 0.83$
$R b^{+} + e^{-} \to R b$ $- 2.93 V$

Use the following from the table and your knowledge of electrochemistry to predict the CORRECT net ionic equation for the reaction that will occur when a molten rubidium chloride undergoes electrolysis.

2 R b^{+} + 2 C l^{-} \to 2 R b + C l_{2}

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2 H_{2} O \to 2 H_{2} + O_{2}

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H_{2} + 2 O H^{-} + 2 R b^{+} \to 2 R b + 2 H_{2} O

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4 C l^{-} + O_{2} + 4 H^{+} \to 2 H_{2} O + 2 C l_{2}

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Solution

The correct option is B $2 R b^{+} + 2 C l^{-} \to 2 R b + C l_{2}$
From the given table, we have;
Rb as the lowest reduction potential, therefore, it undergoes oxidation and $C l_{2}$ have the reduction potential, therefore, it undergoes reduction.

So, the net cell reaction becomes:

$2 R b + C l_{2} \to 2 R b^{+} + 2 C l^{-}$

When the molten rubidium chloride undergoes electrolysis the reaction gets reversed.

$2 R b^{+} + 2 C l^{-} \to 2 R b + C l_{2}$

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Similar questions

Q. Consider the table of standard reduction potentials shown below.

Half-reaction	$E^{\circ}$
$C l_{2} + 2 e^{-} \to 2 C l^{-}$	$1.36 V$
$O_{2} + 4 H^{+} + 4 e^{-} \to 2 H_{2} O$	$1.23 V$
$2 H_{2} O + 2 e^{-} \to H_{2} + 2 O H^{-}$	$- 0.83 V$
$R b^{+} + e^{-} \to R b$	$- 2.93 V$

Use the information from the table and your knowledge of electrochemistry to predict the CORRECT net ionic equation for the reaction that will occur when an aqueous solution of rubidium chloride undergoes electrolysis.

Q. Consider the following reactions:
I.

2 N a + 2 H_{2} O \to 2 N a O H + H_{2}

II.

2 N a O H + C l_{2} \to N a C l + N a O C l + H_{2} O

III.

4 O H^{-} \to O_{2} + 2 H_{2} O + 4 e^{-}

IV.

2 C l^{-} \to C l_{2} + 2 e^{-}

In the diaphragm cell used for the electrolysis of brine, the reactions that occur would include :

Q. Given are the reactions occuring during the electrolysis of sodium chloride solution:

$2 C l^{-} \to C l_{2} + 2 e^{-}$
$2 H_{2} O + 2 e^{-} \to H_{2} + 2 O H^{-}$

Which of the following is correct regarding liberation of electrolytic products?

Q. Cathode:

{2 H}_{2} O + {2 e}^{-} \to H_{2} + 2 {O H}^{-}

Anode:

{x O H}^{-} \to O_{2} + {2 H}_{2} O + {y e}^{-}

Overall:

{2 H}_{2} O \to 2 H_{2} + O_{2}

Find the value of x and y:

Q. Rank the following elements by increasing ease of oxidation with most easily oxidized LAST:

C d, C u, N i, F e

Standard Reduction Potentials at

25^{\circ} C

Half-Reaction	$E^{\circ} (V)$
$F_{2} + 2 e^{-} \to 2 F^{-}$	$2.87$
$A g^{2} + e^{-} \to A g^{+}$	$1.99$
$C o^{3 +} + e^{-} \to C o^{2 +}$	$1.82$
$H_{2} O_{2} + 2 H^{+} + 2 e^{-} \to 2 H_{2} O$	$1.78$
$M n O_{4}^{-} + 4 H^{+} + 3 e^{-} \to M n O_{2} + 2 H_{2} O$	$1.68$
$2 e^{-} + 2 H^{+} + I O_{4}^{-} \to I O_{3}^{-} + H_{2} O$	$1.60$
$M n O_{4}^{-} + 8 H^{+} + 5 e^{-} \to M n^{2 +} + 4 H_{2} O$	$1.51$
$A u^{3 +} + 3 e^{-} \to A u$	$1.50$
$C l_{2} + 2 e^{-} \to 2 C l^{-}$	$1.36$
$O_{2} + 4 H^{+} + 4 e^{-} \to 2 H_{2} O$	$1.23$
$M n O_{2} + 4 H^{+} + 2 e^{-} \to M n^{2 +} + 2 H_{2} O$	$1.21$
$B r_{2} + 2 e^{-} \to 2 B r^{-}$	$1.09$
$N O_{3}^{-} + 4 H^{+} + 3 e^{-} \to N O + 2 H_{2} O$	$0.96$
$C l O_{2} + e^{-} \to C l O_{2}$	$0.954$
$2 H g^{2 +} + 2 e^{-} \to H g_{2}^{2 +}$	$0.91$
$A g^{+} + e^{-} \to A g$	$0.80$
$H g_{2}^{2 +} + 2 e^{-} \to 2 H g$	$0.80$
$F e^{3 +} + e^{-} \to F e^{2 +}$	$0.77$
$O_{2} + 2 H^{+} + 2 e^{-} \to H_{2} O_{2}$	$0.68$
$M n O_{4}^{-} + e^{-} \to M n O_{4}^{2 -}$	$0.56$
$I_{2} + 2 e^{-} \to 2 I^{-}$	$0.54$
$C u^{+} + e^{-} \to C u$	$0.52$
$O_{2} + 2 H_{2} O + 4 e^{-} \to 4 O H^{-}$	$0.40$
$C u^{2 +} + 2 e^{-} \to C u$	$0.34$
$A g C l + e^{-} \to A g + C l^{-}$	$0.22$
$C u^{2 +} + e^{-} \to C u^{+}$	$0.16$
$2 H^{+} + 2 e^{-} \to H_{2}$	$0.00$
$F e^{3 +} + 3 e^{-} \to F e$	$- 0.036$
$P b^{2 +} + 2 e^{-} \to P b$	$- 0.13$
$N i^{2 +} + 2 e^{-} \to N i$	$- 0.23$
$C d^{2 +} + 2 e^{-} \to C d$	$- 0.40$
$F e^{2 +} + 2 e^{-} \to F e$	$- 0.44$
$C r^{3 +} + e^{-} \to C r^{2 +}$	$- 0.50$
$C r^{3 +} + 3 e^{-} \to C r$	$- 0.73$
$Z n^{2 +} + 2 e^{-} \to Z n$	$- 0.76$
$2 H_{2} O + 2 e^{-} \to H_{2} + 2 O H^{-}$	$- 0.83$
$M n^{2 +} + 2 e^{-} \to M n$	$- 1.18$
$A l^{3 +} + 3 e^{-} \to A l$	$- 1.66$
$H_{2} + 2 e^{-} \to 2 H^{-}$	$- 2.23$
$M g^{2 +} + 2 e^{-} \to M g$	$- 2.37$
$N a^{+} + e^{-} \to N a$	$- 2.71$
$C a^{2 +} + 2 e^{-} \to C a$	$- 2.76$
$B a^{2 +} + 2 e^{-} \to B a$	$- 2.90$
$K^{+} + e^{-} \to K$	$- 2.92$
$L i^{+} + e^{-} \to L i$	$- 3.05$

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