For the given reaction: CaCO3 + 2HCl - CaCl2 + H2O + CO2 If 90 g CaCO3 is added to 300 mL of HCl which contai…

Question

For the given reaction: $$\ce{CaCO3 + 2HCl -> CaCl2 + H2O + CO2}$$
If **$$90 \, 	ext{g}$$** $$\ce{CaCO3}$$ is added to **$$300 \, 	ext{mL}$$** of $$\ce{HCl}$$ which contains **$$38.55\%$$** $$\ce{HCl}$$ by mass and has density **$$1.13 \, 	ext{g mL}^{-1}$$**, then which of the following option is correct?

Given molar mass of **H**, **Cl**, **Ca** and **O** are **$$1$$**, **$$35.5$$**, **$$40$$** and **$$16 \, 	ext{g mol}^{-1}$$** respectively.

Accepted Answer

D. **$$64.97 \, 	ext{g}$$** of $$\ce{HCl}$$ remains unreacted

Answer

A. **$$60.32 \, 	ext{g}$$** of $$\ce{HCl}$$ remains unreacted

Answer

B. **$$32.85 \, 	ext{g}$$** of $$\ce{CaCO_3}$$ remains unreacted

Answer

C. **$$97.30 \, 	ext{g}$$** of $$\ce{HCl}$$ reacted

Answer & step-by-step solution

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