Hey please help me with this question!
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Here's the answer correctly:
The reaction taking place in the question:
At anode: Mn2+(aq) + 2H2O(L) --> MnO2(s) + 4H(aq) 2e-
At cathode: 2H+(aq) + 2e --> H2(g)
Overall reaction: Mn2(aq) + 2H2O(l) --> MnO2(s) + 2H+(aq) + H2(g)
Amount of current is given by -
I = m . FxZ/txM
Where m is the weight of MnO2 = 1kg = 1000g[given]
F= Faraday's constant
t= time required
Z= no. of electrons transferred
M= mass of Mn02 = (55+32)= 87 g/mol
Substituting these values, we get:
I = 1000 g [ 95600C/mol x 2/24x60x60x87]
= 25.67 A
Now current efficiency = 25.67/27 x 100% = 95.07% = 95%
Hence the answer is option B.
The reaction taking place in the question:
At anode: Mn2+(aq) + 2H2O(L) --> MnO2(s) + 4H(aq) 2e-
At cathode: 2H+(aq) + 2e --> H2(g)
Overall reaction: Mn2(aq) + 2H2O(l) --> MnO2(s) + 2H+(aq) + H2(g)
Amount of current is given by -
I = m . FxZ/txM
Where m is the weight of MnO2 = 1kg = 1000g[given]
F= Faraday's constant
t= time required
Z= no. of electrons transferred
M= mass of Mn02 = (55+32)= 87 g/mol
Substituting these values, we get:
I = 1000 g [ 95600C/mol x 2/24x60x60x87]
= 25.67 A
Now current efficiency = 25.67/27 x 100% = 95.07% = 95%
Hence the answer is option B.
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