Question 13:How much electricity in terms of Faraday is required to produce (i) 20.0 g of Ca from molten CaCl2. (ii) 40.0 g of Al from molten Al2O3. Chapter 3: Electrochemistry Chemistry Class 12 solutions are developed for assisting understudies with working on their score and increase knowledge of the subjects. How much electricity in terms of Faraday is required to produce (i) 20.0 g of Ca from molten CaCl2. (ii) 40.0 g of Al from molten Al2O3. is solved by our expert teachers. You can get ncert solutions and notes for class 12 chapter 3 absolutely free. NCERT Solutions for class 12 Chemistry Chapter 3: Electrochemistry is very essencial for getting good marks in CBSE Board examinations
Question 13:How much electricity in terms of Faraday is required to produce
(i) 20.0 g of Ca from molten CaCl2.
(ii) 40.0 g of Al from molten Al2O3.
Answer:(i)
The balance reaction will
The charge on Ca in CaCl2
Ca + 2Cl = 0
Cl has –1 charge so that
Ca + 2(–1) = 0
Ca = 2
We have to get 2o g Ca from Ca2+
Number of required moles = mass / molar mass
Molar mass of Ca is 40 g/mol and required mass of Ca is 20 g
Hence number of moles = 20/40 = 0.5 mol
Electricity required to produce 1 mol of calcium = 2 F
The electricity required to produce 0.5 mol of calcium
= 0.5 × 2 F
= 1 F
(ii)
Charge on Al in Al2O3
2Al + 3O = 0
Oxygen has –2
2Al +3(–2) = 0
Al = 3
Change transfer n = 3
Charge required for 1 mol of Al = 3F
Number of moles of Al = 40 /27 = 1.48
The electricity required to produce 1.48 mol of Al = 1.48 × 3 F
= 4.44 F
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