Chemical BondingHard
Question
Which of the following statements is/are correct ?
Commercial HCl is prepared by heating NaCl with H2SO4.
2NaCl + H2SO4 → N2SO4 + 2HCl
Commercial HCl is prepared by heating NaCl with H2SO4.
2NaCl + H2SO4 → N2SO4 + 2HCl
Options
A.196.0 g of pure H2SO4 is required for thr production of 245.0 g of cone HCl containing 40% HCl by weight
B.245.0 g of 80% H2SO4 by weight is required for the production of 365.0 g of cone. HCl containing 40% HCl by weight.
C.2 mol of pure H2SO4 is required for the production of 365 g of 40% HCl.
D.2.5 mol of 80% H2SO4 is required for the production of 365.0 g of 40% HCl.
Solution
a. Weight of 40% HCl = 
× 36.5 = 146 g
2 mol HCl (2 × 36.5 = 73 g) = 1 mol H2SO4 (98g)
Weight of H2SO4 = (146 g HCl)
= 196 g H2SO4.
b. Weight of 80% H2SO4
=
= 245 g H2SO4
c. Mole of pure H2SO4
=
= 2 mol H2SO4
d. Mole of 80% H2SO4 =
= 2.5 mol H2SO4
× 36.5 = 146 g2 mol HCl (2 × 36.5 = 73 g) = 1 mol H2SO4 (98g)
Weight of H2SO4 = (146 g HCl)
= 196 g H2SO4.
b. Weight of 80% H2SO4
=
= 245 g H2SO4c. Mole of pure H2SO4
=
= 2 mol H2SO4d. Mole of 80% H2SO4 =
= 2.5 mol H2SO4Create a free account to view solution
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