How much electricity in terms of Faraday is required to produce .
(i) 20.0 g of Ca from molten `CaCl_(2)`
(ii) 40.0 g of Al form molten`Al_(2)O_(3)` .

What volume of H_(2) at STP is required to reduce 0.795 g of CuO to give Cu and H_(2)O .

How much electricity is required in coulomb for the oxidation of (i) 1 mol of H_(2)O to O_(2) . (ii) mol of FeO to Fe_(2)O_(3) .

How many grams of Al_2(SO_4)_3 , will be required to prepare 4 litres of 0.025M solution ?

How much charge is required for the following reductions: (i) 1 mol of Al^(3+) to Al. (ii) 1 mol of Cu^(2+) to Cu. (iii) 1 mol of MnO_(4)^(-) to Mn^(2+) .

The volume of 0.1 M HCl required in mL to neutralise 20 mL of a solution containing 0.106 g of Na_(2)CO_(3) is

In the reactions given below, identify the species undergoing oxidation and reduction : (i) H_(2)S (g) + Cl_(2) (g) rarr HCl (g) + S (s) (ii) 3Fe_(3)O_(4) (s) + 8 Al (s) rarr 9 Fe(s) + 4Al_(2)O_(3) (s) (iii) 2Na (s) + H_(2) (g) rarr 2 NaH (s)

During Aluminothermy one mole of Cr_(2)O_(3) reduced to Cr. How many no. of the moles of Al required.

When electricity is passed through molten AlCl_3 , 13.5 g. of Al is deposited. The number of Faradays must be

The number of moles of H_(2) which is required to produce 10 moles of NH_(3) in the following reaction is aH_(2)(g)+bNO_(2)(g)tocNH_(3)(g)+dH_(2)O(g)