ElectrochemistryHard
Question
Perdisulphuric acid, H2S2O8 can be prepared by electrolytic oxidation of H2SO4, oxygen and hydrogen gases are by products. In such an electrolysis, 9.08 L of H2 and 2.27 L of O2 were generated at STP. What is the mass of H2S2O8 formed?
Options
A.0
B.77.6 g
C.38.8 g
D.19.4 g
Solution
$n_{eq}H_{2}\left( \text{at Cathode} \right) = n_{eq}O_{2} + n_{eq}H_{2}S_{2}O_{8}\left( \text{at Anode} \right)$
$\text{Or, }\frac{9.08}{22.7} \times 2 = \frac{2.27}{22.7} \times 4 + \frac{w}{194} \times 2\left\lbrack 2SO_{4}^{2 -} \rightarrow S_{2}O_{8}^{2 -} + 2e^{-} \right\rbrack $$$\therefore w = 38.8\text{ gm}$$
Create a free account to view solution
View Solution FreeMore Electrochemistry Questions
After electrolysis of an aqueous sodium chloride solution, it was found that the solution is being neutralized by 60 ml ...Which pure substance will not conduct electricity?...Select the correct option if it is known that Ksp (AgCl) > Ksp (AgBr) > Ksp (AgI)...Two litre solution of a bu er mixture containing 1.0 M – NaH2PO4 and 1.0 M – Na2HPO4 is placed in two compartments (one ...Pure water is saturated with pure solid AgCl, a silver electrode is placed in the solution and the potential is measured...