Answer:
There are needed 198g of Ca to react completely with 2.20L of a 4.50M HCl solution
Explanation:
First we need to establish the chemical reaction between Ca and HCl.
Ca + HCl → CaCl₂ + H₂
Then we need to balance the equation to find out the stoichiometry of the reaccion, to do this we need to keep in count that in a chemical reaction mass cannot be generated or created, so the reactants must have the same amount of mass as the product
The balanced equation is:
Ca + 2HCl → CaCl₂ + H₂
This means that 1 mol of Ca reacts with 2 moles of HCl to form 1 mol of CaCl₂ and 1 mol of H₂.
Next we need to find out how many moles we have in the solution.
1L of solution ⇒ 4.50 moles of HCl
2.20L of solution ⇒ x moles of HCl
[tex]x = \frac{2.20L · 4.50 mol}{1L}[/tex]
x = 9.9 moles of HCl
Now we use the stoichiometric ratio between HCl a Ca to find out how many moles react with 9.9 moles of HCl.
2 moles of HCl ⇒ 1 mol of Ca
9.9 moles of HCl ⇒ x moles of Ca
[tex]x = \frac{9.9 mol· 1 mol}{2mol}[/tex]
x = 4.95 moles of Ca
Finally we calculate how many grams 4.95 moles of Ca are, using the Ca molar mass.
1 mol of Ca ⇒ 40g
4.95 moles of Ca ⇒ x g
[tex]x = \frac{4.95 mol ·40g}{1 mol}[/tex]
x = 198g
