For the given reaction; CaCO3 + 2HC1 CaCl2 + H2O + CO2 If 90 g CaCO3 is added to 300 mL of HCl which contains 38.55% HCl by mass and has density 1.13 g mL –1, then which of the following option is cor

Question

For the given reaction; CaCO3 + 2HC1 CaCl2 + H2O + CO2 If 90 g CaCO3 is added to 300 mL of HCl which contains 38.55% HCl by mass and has density 1.13 g mL –1, then which of the following option is correct? Given molar mass of H, Cl, Ca and O are 1, 35.5, 40 and 16 g mol –1 respectively.

(A) 64.97 g of HCl remains unreacted
(B) 32.85 g of CaCO3 remains unreacted
(C) 97.30 g of HCl reacted
(D) 60.32 g of HCl reamains unreacted

Prashant Kotian · Accepted Answer

Correct answer: A. Density of HCl solution (d) =1.13g/ml V=300ml Wt. of HCl solution = 339 g Wt. of HCl = 339 × 38.55 100 = 130.68 g (LR) CaCO3 + 2HCl  CaCl2 + H2O + CO2 100 130.68 36.5 =0.90mole = 3.58 mole Moles of HCl remained = 1.78 mole. Mass of HCl remained = 64.97 g.

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