330258
If an aqueous \(\mathrm{NaCl}\) solution is electrolysed using a current of \(5 \mathrm{~A}\) for \(200 \mathrm{~min}\). Volume of \(\mathrm{Cl}_{2}(\mathrm{~g})\) in litres produced under STP condition is \(({\rm{F}} = 96000\,\,{\rm{C}}).\)
330259
How many Faradays of electricity are required to oxidize 1 mol of water to dioxygen?
1 4
2 2
3 1
4 3
Explanation:
\({\mathrm{\mathrm{H}_{2} \mathrm{O} \longrightarrow 2 \mathrm{H}^{+}+2 \mathrm{e}^{-}+\dfrac{1}{2} \mathrm{O}_{2}}}\) Hence, for the oxidation of one mole of water to dioxygen, 2 moles of electrons \({\mathrm{=2 \mathrm{~F}}}\) electricity is required.
CHXII03:ELECTROCHEMISTRY
330260
Which one of the following statements is correct for electrolysis of brine solution?
1 \(\mathrm{OH}^{-}\) is formed at cathode.
2 \(\mathrm{Cl}_{2}\) is formed at cathode.
3 \(\mathrm{O}_{2}\) is formed at cathode.
4 \(\mathrm{H}_{2}\) is formed at anode.
Explanation:
Statement 4 is incorrect. \(\mathrm{H}_{2}\) is formed at cathode . \(\mathrm{NaCl}_{(\mathrm{aq})} \rightarrow \mathrm{Na}^{+}+\mathrm{Cl}^{-}\) Cathode reaction:\(2 \mathrm{H}_{2} \mathrm{O}+2 \mathrm{e}^{-} \xrightarrow{\text { reduction }} \mathrm{H}_{2(\mathrm{~g})}+2 \mathrm{OH}^{-}\) Anode reaction : \(2 \mathrm{Cl}^{-} \xrightarrow{\text { reduction }} \mathrm{Cl}_{2(\mathrm{~g})}+2 \mathrm{e}^{-}\)
330258
If an aqueous \(\mathrm{NaCl}\) solution is electrolysed using a current of \(5 \mathrm{~A}\) for \(200 \mathrm{~min}\). Volume of \(\mathrm{Cl}_{2}(\mathrm{~g})\) in litres produced under STP condition is \(({\rm{F}} = 96000\,\,{\rm{C}}).\)
330259
How many Faradays of electricity are required to oxidize 1 mol of water to dioxygen?
1 4
2 2
3 1
4 3
Explanation:
\({\mathrm{\mathrm{H}_{2} \mathrm{O} \longrightarrow 2 \mathrm{H}^{+}+2 \mathrm{e}^{-}+\dfrac{1}{2} \mathrm{O}_{2}}}\) Hence, for the oxidation of one mole of water to dioxygen, 2 moles of electrons \({\mathrm{=2 \mathrm{~F}}}\) electricity is required.
CHXII03:ELECTROCHEMISTRY
330260
Which one of the following statements is correct for electrolysis of brine solution?
1 \(\mathrm{OH}^{-}\) is formed at cathode.
2 \(\mathrm{Cl}_{2}\) is formed at cathode.
3 \(\mathrm{O}_{2}\) is formed at cathode.
4 \(\mathrm{H}_{2}\) is formed at anode.
Explanation:
Statement 4 is incorrect. \(\mathrm{H}_{2}\) is formed at cathode . \(\mathrm{NaCl}_{(\mathrm{aq})} \rightarrow \mathrm{Na}^{+}+\mathrm{Cl}^{-}\) Cathode reaction:\(2 \mathrm{H}_{2} \mathrm{O}+2 \mathrm{e}^{-} \xrightarrow{\text { reduction }} \mathrm{H}_{2(\mathrm{~g})}+2 \mathrm{OH}^{-}\) Anode reaction : \(2 \mathrm{Cl}^{-} \xrightarrow{\text { reduction }} \mathrm{Cl}_{2(\mathrm{~g})}+2 \mathrm{e}^{-}\)
330258
If an aqueous \(\mathrm{NaCl}\) solution is electrolysed using a current of \(5 \mathrm{~A}\) for \(200 \mathrm{~min}\). Volume of \(\mathrm{Cl}_{2}(\mathrm{~g})\) in litres produced under STP condition is \(({\rm{F}} = 96000\,\,{\rm{C}}).\)
330259
How many Faradays of electricity are required to oxidize 1 mol of water to dioxygen?
1 4
2 2
3 1
4 3
Explanation:
\({\mathrm{\mathrm{H}_{2} \mathrm{O} \longrightarrow 2 \mathrm{H}^{+}+2 \mathrm{e}^{-}+\dfrac{1}{2} \mathrm{O}_{2}}}\) Hence, for the oxidation of one mole of water to dioxygen, 2 moles of electrons \({\mathrm{=2 \mathrm{~F}}}\) electricity is required.
CHXII03:ELECTROCHEMISTRY
330260
Which one of the following statements is correct for electrolysis of brine solution?
1 \(\mathrm{OH}^{-}\) is formed at cathode.
2 \(\mathrm{Cl}_{2}\) is formed at cathode.
3 \(\mathrm{O}_{2}\) is formed at cathode.
4 \(\mathrm{H}_{2}\) is formed at anode.
Explanation:
Statement 4 is incorrect. \(\mathrm{H}_{2}\) is formed at cathode . \(\mathrm{NaCl}_{(\mathrm{aq})} \rightarrow \mathrm{Na}^{+}+\mathrm{Cl}^{-}\) Cathode reaction:\(2 \mathrm{H}_{2} \mathrm{O}+2 \mathrm{e}^{-} \xrightarrow{\text { reduction }} \mathrm{H}_{2(\mathrm{~g})}+2 \mathrm{OH}^{-}\) Anode reaction : \(2 \mathrm{Cl}^{-} \xrightarrow{\text { reduction }} \mathrm{Cl}_{2(\mathrm{~g})}+2 \mathrm{e}^{-}\)
330258
If an aqueous \(\mathrm{NaCl}\) solution is electrolysed using a current of \(5 \mathrm{~A}\) for \(200 \mathrm{~min}\). Volume of \(\mathrm{Cl}_{2}(\mathrm{~g})\) in litres produced under STP condition is \(({\rm{F}} = 96000\,\,{\rm{C}}).\)
330259
How many Faradays of electricity are required to oxidize 1 mol of water to dioxygen?
1 4
2 2
3 1
4 3
Explanation:
\({\mathrm{\mathrm{H}_{2} \mathrm{O} \longrightarrow 2 \mathrm{H}^{+}+2 \mathrm{e}^{-}+\dfrac{1}{2} \mathrm{O}_{2}}}\) Hence, for the oxidation of one mole of water to dioxygen, 2 moles of electrons \({\mathrm{=2 \mathrm{~F}}}\) electricity is required.
CHXII03:ELECTROCHEMISTRY
330260
Which one of the following statements is correct for electrolysis of brine solution?
1 \(\mathrm{OH}^{-}\) is formed at cathode.
2 \(\mathrm{Cl}_{2}\) is formed at cathode.
3 \(\mathrm{O}_{2}\) is formed at cathode.
4 \(\mathrm{H}_{2}\) is formed at anode.
Explanation:
Statement 4 is incorrect. \(\mathrm{H}_{2}\) is formed at cathode . \(\mathrm{NaCl}_{(\mathrm{aq})} \rightarrow \mathrm{Na}^{+}+\mathrm{Cl}^{-}\) Cathode reaction:\(2 \mathrm{H}_{2} \mathrm{O}+2 \mathrm{e}^{-} \xrightarrow{\text { reduction }} \mathrm{H}_{2(\mathrm{~g})}+2 \mathrm{OH}^{-}\) Anode reaction : \(2 \mathrm{Cl}^{-} \xrightarrow{\text { reduction }} \mathrm{Cl}_{2(\mathrm{~g})}+2 \mathrm{e}^{-}\)
330258
If an aqueous \(\mathrm{NaCl}\) solution is electrolysed using a current of \(5 \mathrm{~A}\) for \(200 \mathrm{~min}\). Volume of \(\mathrm{Cl}_{2}(\mathrm{~g})\) in litres produced under STP condition is \(({\rm{F}} = 96000\,\,{\rm{C}}).\)
330259
How many Faradays of electricity are required to oxidize 1 mol of water to dioxygen?
1 4
2 2
3 1
4 3
Explanation:
\({\mathrm{\mathrm{H}_{2} \mathrm{O} \longrightarrow 2 \mathrm{H}^{+}+2 \mathrm{e}^{-}+\dfrac{1}{2} \mathrm{O}_{2}}}\) Hence, for the oxidation of one mole of water to dioxygen, 2 moles of electrons \({\mathrm{=2 \mathrm{~F}}}\) electricity is required.
CHXII03:ELECTROCHEMISTRY
330260
Which one of the following statements is correct for electrolysis of brine solution?
1 \(\mathrm{OH}^{-}\) is formed at cathode.
2 \(\mathrm{Cl}_{2}\) is formed at cathode.
3 \(\mathrm{O}_{2}\) is formed at cathode.
4 \(\mathrm{H}_{2}\) is formed at anode.
Explanation:
Statement 4 is incorrect. \(\mathrm{H}_{2}\) is formed at cathode . \(\mathrm{NaCl}_{(\mathrm{aq})} \rightarrow \mathrm{Na}^{+}+\mathrm{Cl}^{-}\) Cathode reaction:\(2 \mathrm{H}_{2} \mathrm{O}+2 \mathrm{e}^{-} \xrightarrow{\text { reduction }} \mathrm{H}_{2(\mathrm{~g})}+2 \mathrm{OH}^{-}\) Anode reaction : \(2 \mathrm{Cl}^{-} \xrightarrow{\text { reduction }} \mathrm{Cl}_{2(\mathrm{~g})}+2 \mathrm{e}^{-}\)