Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCI(aq), as described by the chemical equation MnO,(s) + 4 HCl(aq) → MNCI, (aq) + 2 H,O(1) + Cl,(g) How much MnO, (s) should be added to excess HCl(aq) to obtain 105 mL of Cl,(g) at 25 °C and 715 Torr? (Hint: It's another stoichiometry problem. See hints for previous problems. You will get n which is moles of chlorine gas first, then use stoichiometry to get moles of the reactant that you need, then grams of that reactant.) g MnO, mass:

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**Stoichiometry Problem: Preparing Chlorine in the Laboratory**

Chlorine can be prepared in the laboratory by the reaction of manganese dioxide (\( \text{MnO}_2 \)) with hydrochloric acid (\( \text{HCl(aq)} \)), as described by the chemical equation:

\[ \text{MnO}_2(s) + 4 \text{HCl(aq)} \rightarrow \text{MnCl}_2(aq) + 2 \text{H}_2\text{O}(l) + \text{Cl}_2(g) \]

**Problem:**  
How much \( \text{MnO}_2(s) \) should be added to excess \( \text{HCl(aq)} \) to obtain 105 mL of \( \text{Cl}_2(g) \) at 25 °C and 715 Torr?

**Hint:** It's another stoichiometry problem. See hints for previous problems. You will first determine \( n \), which represents moles of chlorine gas. Then, use stoichiometry to calculate moles of the reactant needed. Finally, convert this to grams of that reactant.

**Calculation:**  
\[ \text{Mass:} \ \_\_\_\_\_\_\ \text{g MnO}_2 \]
Transcribed Image Text:**Stoichiometry Problem: Preparing Chlorine in the Laboratory** Chlorine can be prepared in the laboratory by the reaction of manganese dioxide (\( \text{MnO}_2 \)) with hydrochloric acid (\( \text{HCl(aq)} \)), as described by the chemical equation: \[ \text{MnO}_2(s) + 4 \text{HCl(aq)} \rightarrow \text{MnCl}_2(aq) + 2 \text{H}_2\text{O}(l) + \text{Cl}_2(g) \] **Problem:** How much \( \text{MnO}_2(s) \) should be added to excess \( \text{HCl(aq)} \) to obtain 105 mL of \( \text{Cl}_2(g) \) at 25 °C and 715 Torr? **Hint:** It's another stoichiometry problem. See hints for previous problems. You will first determine \( n \), which represents moles of chlorine gas. Then, use stoichiometry to calculate moles of the reactant needed. Finally, convert this to grams of that reactant. **Calculation:** \[ \text{Mass:} \ \_\_\_\_\_\_\ \text{g MnO}_2 \]
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