Can sulfuric acid itself be electrolysed?Is there anything in the literature that supports revolutionary claims for this “new” sulfuric-acid battery?Prediction of ionic reduction?What is the role of hydrochloric acid in a copper electroplating bath?Reviving a 6 Volt lead-sulfuric acid batteryDoes increasing concentration of copper sulfate decrease or increase its conductivity?How can you identify the anode and cathode of a car battery of indistinct shape by using a potassium iodide solution?Why can higher voltages lead to less efficient electroplating?Lead-Acid Battery: Standard Electrode PotentialWhat are the products in the reaction of sulphuric acid and Group 2 metals?
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Can sulfuric acid itself be electrolysed?
Can sulfuric acid itself be electrolysed?
Is there anything in the literature that supports revolutionary claims for this “new” sulfuric-acid battery?Prediction of ionic reduction?What is the role of hydrochloric acid in a copper electroplating bath?Reviving a 6 Volt lead-sulfuric acid batteryDoes increasing concentration of copper sulfate decrease or increase its conductivity?How can you identify the anode and cathode of a car battery of indistinct shape by using a potassium iodide solution?Why can higher voltages lead to less efficient electroplating?Lead-Acid Battery: Standard Electrode PotentialWhat are the products in the reaction of sulphuric acid and Group 2 metals?
.everyoneloves__top-leaderboard:empty,.everyoneloves__mid-leaderboard:empty,.everyoneloves__bot-mid-leaderboard:empty margin-bottom:0;
$begingroup$
We all could know by now that water can be electrolysed by adding some sulfuric acid.:)
But is it possible that the sulfuric acid itself becomes electrolysed when the concentration of the acid in the water gets higher ?
Would it give sulfur dioxide or sulfur trioxide ?
electrochemistry electrolysis
asked 11 hours ago
ConelisinspaceConelisinspace
1223 bronze badges
$endgroup$
add a comment |
$begingroup$
We all could know by now that water can be electrolysed by adding some sulfuric acid.:)
But is it possible that the sulfuric acid itself becomes electrolysed when the concentration of the acid in the water gets higher ?
Would it give sulfur dioxide or sulfur trioxide ?
electrochemistry electrolysis
asked 11 hours ago
ConelisinspaceConelisinspace
1223 bronze badges
$endgroup$
3
$begingroup$
Rather hydrogen and peroxodisulphuric acid, with ozone as a byproduct. $$ce 2 H2SO4 -> H2 + H2S2O8 $$ en.wikipedia.org/wiki/Peroxydisulfuric_acid
$endgroup$
– Poutnik
10 hours ago
$begingroup$
@Poutnik Thank you for the useful link. I wondered how the sulfuric acid clouds of Venus could be useful.
$endgroup$
– Conelisinspace
10 hours ago
add a comment |
$begingroup$
We all could know by now that water can be electrolysed by adding some sulfuric acid.:)
But is it possible that the sulfuric acid itself becomes electrolysed when the concentration of the acid in the water gets higher ?
Would it give sulfur dioxide or sulfur trioxide ?
electrochemistry electrolysis
asked 11 hours ago
ConelisinspaceConelisinspace
1223 bronze badges
$endgroup$
We all could know by now that water can be electrolysed by adding some sulfuric acid.:)
But is it possible that the sulfuric acid itself becomes electrolysed when the concentration of the acid in the water gets higher ?
Would it give sulfur dioxide or sulfur trioxide ?
electrochemistry electrolysis
electrochemistry electrolysis
asked 11 hours ago
ConelisinspaceConelisinspace
1223 bronze badges
asked 11 hours ago
ConelisinspaceConelisinspace
1223 bronze badges
asked 11 hours ago
ConelisinspaceConelisinspace
1223 bronze badges
asked 11 hours ago
ConelisinspaceConelisinspace
1223 bronze badges
asked 11 hours ago
ConelisinspaceConelisinspace
1223 bronze badges
1223 bronze badges
3
$begingroup$
Rather hydrogen and peroxodisulphuric acid, with ozone as a byproduct. $$ce 2 H2SO4 -> H2 + H2S2O8 $$ en.wikipedia.org/wiki/Peroxydisulfuric_acid
$endgroup$
– Poutnik
10 hours ago
$begingroup$
@Poutnik Thank you for the useful link. I wondered how the sulfuric acid clouds of Venus could be useful.
$endgroup$
– Conelisinspace
10 hours ago
add a comment |
3
$begingroup$
Rather hydrogen and peroxodisulphuric acid, with ozone as a byproduct. $$ce 2 H2SO4 -> H2 + H2S2O8 $$ en.wikipedia.org/wiki/Peroxydisulfuric_acid
$endgroup$
– Poutnik
10 hours ago
$begingroup$
@Poutnik Thank you for the useful link. I wondered how the sulfuric acid clouds of Venus could be useful.
$endgroup$
– Conelisinspace
10 hours ago
3
3
$begingroup$
Rather hydrogen and peroxodisulphuric acid, with ozone as a byproduct. $$ce 2 H2SO4 -> H2 + H2S2O8 $$ en.wikipedia.org/wiki/Peroxydisulfuric_acid
$endgroup$
– Poutnik
10 hours ago
$begingroup$
Rather hydrogen and peroxodisulphuric acid, with ozone as a byproduct. $$ce 2 H2SO4 -> H2 + H2S2O8 $$ en.wikipedia.org/wiki/Peroxydisulfuric_acid
$endgroup$
– Poutnik
10 hours ago
$begingroup$
@Poutnik Thank you for the useful link. I wondered how the sulfuric acid clouds of Venus could be useful.
$endgroup$
– Conelisinspace
10 hours ago
$begingroup$
@Poutnik Thank you for the useful link. I wondered how the sulfuric acid clouds of Venus could be useful.
$endgroup$
– Conelisinspace
10 hours ago
add a comment |
1 Answer
1
active
oldest
votes
$begingroup$
After some searching, I found this 1956 Thesis(Reference), which describes the production of peroxydisulfuric by electrolyzing concentrated sulfuric acid. The yield varied according to the concentration of the acid, temperature, current, and the nature of the electrode. In the Thesis, the chemist noted that discharged $ceHSO4-$ united together to form peroxydisulfuric acid ($ceH2S2O8$). It further stated that oxidation of sulfate ions by anodic oxygen was responsible for the peroxydisulfuric acid formation. Also, hydroxyl ion at anode played an important role in the acid formation.
The reaction mechanism was confirmed by electrolyzing sulfuric acid and ammonium sulfate at various concentration at $pu16!- ! 20 ^circ C$ using platinum electrode and the reaction occurred in accordance to the theory. It was also confirmed that amount of peroxidic oxygen increased with increase in ammonium sulfate. The specific gravity of sulfuric acid and the current density was varied and accordingly the highest yield of 78.4% was obtained. It was also noted that increasing the current density increases the yield up to a certain point as peroxydisulfuric acid was found to convert into peroxymonosulfuric acid. At that moment, a small trace of hydrogen peroxide was noted.
So, the chemical species formed during electrolysis are $ceHSO4-$, $ceSO4^2-$, peroxide ion, protons, trace of hydrogen peroxide, and other side products.
Reference:
Sin-Chou Fan, “The electrolytic production of peroxydisulfuric acid using periodically reversed direct current and alternating current superimposed on direct current,” MS Thesis, Virginia Polytechnic Institute, 1956.
edited 9 hours ago
Mathew Mahindaratne
10.9k1 gold badge13 silver badges39 bronze badges
answered 9 hours ago
Nilay GhoshNilay Ghosh
10.3k10 gold badges47 silver badges112 bronze badges
$endgroup$
add a comment |
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1 Answer
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$begingroup$
After some searching, I found this 1956 Thesis(Reference), which describes the production of peroxydisulfuric by electrolyzing concentrated sulfuric acid. The yield varied according to the concentration of the acid, temperature, current, and the nature of the electrode. In the Thesis, the chemist noted that discharged $ceHSO4-$ united together to form peroxydisulfuric acid ($ceH2S2O8$). It further stated that oxidation of sulfate ions by anodic oxygen was responsible for the peroxydisulfuric acid formation. Also, hydroxyl ion at anode played an important role in the acid formation.
The reaction mechanism was confirmed by electrolyzing sulfuric acid and ammonium sulfate at various concentration at $pu16!- ! 20 ^circ C$ using platinum electrode and the reaction occurred in accordance to the theory. It was also confirmed that amount of peroxidic oxygen increased with increase in ammonium sulfate. The specific gravity of sulfuric acid and the current density was varied and accordingly the highest yield of 78.4% was obtained. It was also noted that increasing the current density increases the yield up to a certain point as peroxydisulfuric acid was found to convert into peroxymonosulfuric acid. At that moment, a small trace of hydrogen peroxide was noted.
So, the chemical species formed during electrolysis are $ceHSO4-$, $ceSO4^2-$, peroxide ion, protons, trace of hydrogen peroxide, and other side products.
Reference:
Sin-Chou Fan, “The electrolytic production of peroxydisulfuric acid using periodically reversed direct current and alternating current superimposed on direct current,” MS Thesis, Virginia Polytechnic Institute, 1956.
edited 9 hours ago
Mathew Mahindaratne
10.9k1 gold badge13 silver badges39 bronze badges
answered 9 hours ago
Nilay GhoshNilay Ghosh
10.3k10 gold badges47 silver badges112 bronze badges
$endgroup$
add a comment |
$begingroup$
After some searching, I found this 1956 Thesis(Reference), which describes the production of peroxydisulfuric by electrolyzing concentrated sulfuric acid. The yield varied according to the concentration of the acid, temperature, current, and the nature of the electrode. In the Thesis, the chemist noted that discharged $ceHSO4-$ united together to form peroxydisulfuric acid ($ceH2S2O8$). It further stated that oxidation of sulfate ions by anodic oxygen was responsible for the peroxydisulfuric acid formation. Also, hydroxyl ion at anode played an important role in the acid formation.
The reaction mechanism was confirmed by electrolyzing sulfuric acid and ammonium sulfate at various concentration at $pu16!- ! 20 ^circ C$ using platinum electrode and the reaction occurred in accordance to the theory. It was also confirmed that amount of peroxidic oxygen increased with increase in ammonium sulfate. The specific gravity of sulfuric acid and the current density was varied and accordingly the highest yield of 78.4% was obtained. It was also noted that increasing the current density increases the yield up to a certain point as peroxydisulfuric acid was found to convert into peroxymonosulfuric acid. At that moment, a small trace of hydrogen peroxide was noted.
So, the chemical species formed during electrolysis are $ceHSO4-$, $ceSO4^2-$, peroxide ion, protons, trace of hydrogen peroxide, and other side products.
Reference:
Sin-Chou Fan, “The electrolytic production of peroxydisulfuric acid using periodically reversed direct current and alternating current superimposed on direct current,” MS Thesis, Virginia Polytechnic Institute, 1956.
edited 9 hours ago
Mathew Mahindaratne
10.9k1 gold badge13 silver badges39 bronze badges
answered 9 hours ago
Nilay GhoshNilay Ghosh
10.3k10 gold badges47 silver badges112 bronze badges
$endgroup$
add a comment |
$begingroup$
After some searching, I found this 1956 Thesis(Reference), which describes the production of peroxydisulfuric by electrolyzing concentrated sulfuric acid. The yield varied according to the concentration of the acid, temperature, current, and the nature of the electrode. In the Thesis, the chemist noted that discharged $ceHSO4-$ united together to form peroxydisulfuric acid ($ceH2S2O8$). It further stated that oxidation of sulfate ions by anodic oxygen was responsible for the peroxydisulfuric acid formation. Also, hydroxyl ion at anode played an important role in the acid formation.
The reaction mechanism was confirmed by electrolyzing sulfuric acid and ammonium sulfate at various concentration at $pu16!- ! 20 ^circ C$ using platinum electrode and the reaction occurred in accordance to the theory. It was also confirmed that amount of peroxidic oxygen increased with increase in ammonium sulfate. The specific gravity of sulfuric acid and the current density was varied and accordingly the highest yield of 78.4% was obtained. It was also noted that increasing the current density increases the yield up to a certain point as peroxydisulfuric acid was found to convert into peroxymonosulfuric acid. At that moment, a small trace of hydrogen peroxide was noted.
So, the chemical species formed during electrolysis are $ceHSO4-$, $ceSO4^2-$, peroxide ion, protons, trace of hydrogen peroxide, and other side products.
Reference:
Sin-Chou Fan, “The electrolytic production of peroxydisulfuric acid using periodically reversed direct current and alternating current superimposed on direct current,” MS Thesis, Virginia Polytechnic Institute, 1956.
edited 9 hours ago
Mathew Mahindaratne
10.9k1 gold badge13 silver badges39 bronze badges
answered 9 hours ago
Nilay GhoshNilay Ghosh
10.3k10 gold badges47 silver badges112 bronze badges
$endgroup$
After some searching, I found this 1956 Thesis(Reference), which describes the production of peroxydisulfuric by electrolyzing concentrated sulfuric acid. The yield varied according to the concentration of the acid, temperature, current, and the nature of the electrode. In the Thesis, the chemist noted that discharged $ceHSO4-$ united together to form peroxydisulfuric acid ($ceH2S2O8$). It further stated that oxidation of sulfate ions by anodic oxygen was responsible for the peroxydisulfuric acid formation. Also, hydroxyl ion at anode played an important role in the acid formation.
The reaction mechanism was confirmed by electrolyzing sulfuric acid and ammonium sulfate at various concentration at $pu16!- ! 20 ^circ C$ using platinum electrode and the reaction occurred in accordance to the theory. It was also confirmed that amount of peroxidic oxygen increased with increase in ammonium sulfate. The specific gravity of sulfuric acid and the current density was varied and accordingly the highest yield of 78.4% was obtained. It was also noted that increasing the current density increases the yield up to a certain point as peroxydisulfuric acid was found to convert into peroxymonosulfuric acid. At that moment, a small trace of hydrogen peroxide was noted.
So, the chemical species formed during electrolysis are $ceHSO4-$, $ceSO4^2-$, peroxide ion, protons, trace of hydrogen peroxide, and other side products.
Reference:
Sin-Chou Fan, “The electrolytic production of peroxydisulfuric acid using periodically reversed direct current and alternating current superimposed on direct current,” MS Thesis, Virginia Polytechnic Institute, 1956.
edited 9 hours ago
Mathew Mahindaratne
10.9k1 gold badge13 silver badges39 bronze badges
answered 9 hours ago
Nilay GhoshNilay Ghosh
10.3k10 gold badges47 silver badges112 bronze badges
edited 9 hours ago
Mathew Mahindaratne
10.9k1 gold badge13 silver badges39 bronze badges
edited 9 hours ago
Mathew Mahindaratne
10.9k1 gold badge13 silver badges39 bronze badges
edited 9 hours ago
Mathew Mahindaratne
10.9k1 gold badge13 silver badges39 bronze badges
10.9k1 gold badge13 silver badges39 bronze badges
answered 9 hours ago
Nilay GhoshNilay Ghosh
10.3k10 gold badges47 silver badges112 bronze badges
answered 9 hours ago
Nilay GhoshNilay Ghosh
10.3k10 gold badges47 silver badges112 bronze badges
answered 9 hours ago
Nilay GhoshNilay Ghosh
10.3k10 gold badges47 silver badges112 bronze badges
10.3k10 gold badges47 silver badges112 bronze badges
add a comment |
add a comment |
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3
$begingroup$
Rather hydrogen and peroxodisulphuric acid, with ozone as a byproduct. $$ce 2 H2SO4 -> H2 + H2S2O8 $$ en.wikipedia.org/wiki/Peroxydisulfuric_acid
$endgroup$
– Poutnik
10 hours ago
$begingroup$
@Poutnik Thank you for the useful link. I wondered how the sulfuric acid clouds of Venus could be useful.
$endgroup$
– Conelisinspace
10 hours ago