During electrolysis of molten sodium chloride, the time required to produce 0.1 mole of chlorine gas using a current of 3A is ___________.
- A55 minutes
- ✓107.2 minutes
- C220 minutes
- D330 minutes
Answer: B.
View full solution →258 questions across 9 question groups — pick any mix to generate a Chemistry paper with step-by-step answer keys.
Choose the most appropriate answer from the given alternatives and write the option code and the corresponding answer.
133 Q→02Fill In The Blanks.
20 Q→03Assertion And Reason.
10 Q→04[ 1 MARK QUESTIONS ]
6 Q→05[ 2 Marks Questions ]
29 Q→06Match The Following.
6 Q→07[ 3 Marks Questions ]
31 Q→08[ 5 Marks Questions ]
18 Q→09Find the odd one out
5 Q→One sample from each question group in this chapter. Select any group above to see the full set with answer keys.
Answer: B.
View full solution →Answer: B.
View full solution →Answer: A.
View full solution →Answer: B.
View full solution →| Electrolyte | KCl | $KNO_3$ | HCl | NaOAC | NaCl |
| Λ_(S cm $mol^{-1}$) | 149.9 | 145.0 | 426.2 | 91.0 | 126.5 |
Answer: C.
View full solution →Is it possible to store copper sulphate in an iron vessel for a long time?
Given: $E _{ Cu ^{2+} \mid Cu }^0$ = 0.34 V and $E _{ Fe ^{2+} \mid Fe }^0$ = −0.44 V
A copper electrode is dipped in 0.1 M copper sulphate solution at 25°C. Calculate the electrode potential of copper.
[Given: $E _{ Cu ^{2+} \mid Cu }^0$ = 0.34 V]
| Electrolyte | Battery |
| (i) $NH _4 Cl + ZnCl _2+ H _2 O$ | (a) Mercury button cell |
| (ii) Paste of $KOH$ and $ZnO$ | (b) Lithium - ion battery |
| (iii) $38 \%$ by mass of $H _2 SO _4$ | (c) Leclanche cell |
| (iv) Lithium salt in an organic solvent | (d) Lead storage battery |
| Code: | A | B | C | D |
| $i$. | c | a | d | b |
| ii. | d | c | b | a |
| iii. | a | b | c | d |
| iv. | b | d | a | c |
| (i) $Zn$-anode, Graphite-cathode with $MnO _2$ | (a) Lithium - ion battery reer |
| (ii) $Zn$ amalgamated with mercurry anode, sama $HgO$ mixed with graphite cathode | (b) Leclanche cell |
| (iii) Spongy lead anode, lead plate bearing $PbO _2$ | (c) Mercury button cell |
| (iv) Porous graphite anode, $CoO _2$ cathode | (d) Lead storage battery |
| Code: | A | B | C | D |
| $i$. | b | c | d | b |
| ii. | a | b | b | a |
| iii. | d | a | c | d |
| iv. | c | d | a | c |
| (i) Li-ion battery | (a) Pacemakers |
| (ii) Mercury button cell | (b) Fuel cell |
| (iii) Lead storage battery | (c) Cell phone |
| (iv) $H _2- O _2$ cell | (d) Inverter |
| Code: | A | B | C | D |
| $i$. | a | b | c | d |
| ii. | d | c | b | a |
| iii. | b | d | a | c |
| iv. | c | a | d | b |
| (i) Cell constant | (a) $S m ^2 mol ^{-1}$ |
| (ii) equivalent conductance | (b) $Sm ^{-1}$ |
| (iii) Molar conductance | (c) $Sm ^2 g eq ^{-1}$ |
| (iv) Specific conductance | (d) $m ^{-1}$ |
| Code: | A | B | C | D |
| $i$. | a | b | c | d |
| ii. | d | c | b | a |
| iii. | b | d | a | c |
| iv. | c | a | d | b |
| (i) Resistance | (a) Ohm m |
| (ii) Resistivity | (b) $Sm ^{-1}$ |
| (iii) Conductance | (c) $Ohm$ |
| (iv) Specific conductance | (d) $S$ |
| Code: | A | B | C | D |
| $i$. | a | b | c | d |
| ii. | c | a | d | b |
| iii. | d | c | b | a |
| iv. | b | d | a | c |
The conductivity of a $0.01 M$ solution of a $1: 1$ weak electrolyte at $298 K$ is $1.5 \times 10^{-4} S cm ^{-1}$
i) molar conductivity of the solution
ii) degree of dissociation and the dissociation constant of the weak electrolyte
Given that
$
\begin{aligned}
& \lambda_{\text {cation }}^{\circ}=248.2 S cm ^2 mol ^{-1} \\
& \lambda_{\text {anion }}^{\circ}=51.8 S cm ^2 mol ^{-1}
\end{aligned}
$
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