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The balanced chemical equation provided is:

\[ 2 \, \text{HCl} + \text{Ca(OH)}_2 \rightarrow \text{CaCl}_2 + 2 \, \text{H}_2\text{O} \]

To find how many moles of calcium chloride (\( \text{CaCl}_2 \)) are produced from 6.00 moles of hydrochloric acid (\( \text{HCl} \)), we can use the mole ratio from the balanced equation.

From the equation:
- 2 moles of \( \text{HCl} \) produce 1 mole of \( \text{CaCl}_2 \).

So, the ratio of moles of \( \text{CaCl}_2 \) to \( \text{HCl} \) is 1:2. This means for every 2 moles of \( \text{HCl} \), 1 mole of \( \text{CaCl}_2 \) is produced.

Now, calculate how many moles of \( \text{CaCl}_2 \) are produced from 6.00 moles of \( \text{HCl} \):

\[
\text{Moles of CaCl}_2 = \frac{6.00 \, \text{mol HCl}}{2} = 3.00 \, \text{mol CaCl}_2
\]

Thus, **3.00 moles** of calcium chloride are produced from 6.00 moles of hydrochloric acid.

Would you like further details or have any questions?

Here are some related questions:
1. What would happen if you had 10 moles of \( \text{HCl} \)?
2. How can the stoichiometry be adjusted for different substances in a chemical equation?
3. What other products are formed in this reaction, and how do their amounts relate to \( \text{CaCl}_2 \)?
4. What role does \( \text{Ca(OH)}_2 \) play in this reaction?
5. How would the mole ratio change if the equation were not balanced?

**Tip**: Always ensure the chemical equation is balanced before applying stoichiometric principles.

For the following chemical reaction, how many moles of calcium chloride (CaCl2) are produced from 6.00 mol of hydrochloric acid (HCl)? 2 HCl + Ca(OH)2 → CaCl2 + 2 H2O

Learn how to use stoichiometry to calculate how many moles of calcium chloride (CaCl2) are produced from 6.00 moles of hydrochloric acid (HCl). This chemical equation example is perfect for high school students learning about mole ratios.

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