#### Answer

(a) $CaCO_3 + 2HCl -- \gt CaCl_2 + CO_2 + H_2O$
(b) 5.2 mol $(HCl)$
(c) 2.6 mol $(H_2O)$

#### Work Step by Step

(a) - Write the equation with chemical formulas:
$CaCO_3 + HCl -- \gt CaCl_2 + CO_2 + H_2O$
1. Begin with the elements that appear exactly once in each side:
- Balance the $Cl$:
The subscript for chlorine in the products is "2", from $CaCl_2$. Therefore, we should put a "2" as the coefficient of $HCl$.
$CaCO_3 + 2HCl -- \gt CaCl_2 + CO_2 + H_2O$
- The equation is balanced.
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Use the balance coefficients as conversion factors:
(b) According to the balanced equation, each mole of $CaCO_3$ needs 2 moles of $HCl$ to react:
$2.6 mol (CaCO_3) \times \frac{2mol(HCl)}{1mol(CaCO_3)} = 5.2 mol(HCl)$
(c) According to the balanced equation, each mole of $CaCO_3$ produces one mol of $H_2O$:
$2.6 mol(CaCO_3) \times \frac{1mol(H_2O)}{1mol(CaCO_3)} = 2.6 mol(H_2O)$