How many moles of chlorine are needed to form 46.5 g of sodium fluoride?

\[ \text{Reaction: } \text{Cl}_2(l) + 2\text{NaF}(s) \rightarrow \text{F}_2(g) + 2\text{NaCl}(s) \]

The provided chemical equation indicates there may be an error in the initial question: chlorine is not typically involved in the formation of sodium fluoride. Therefore, the moles of chlorine required can't be calculated.

Explanation:

The student's question revolves around molar relationships in the equation Cl2(l) + 2NaF(s) → F2(g) + 2NaCl(s). However, there seems to be some confusion as the byproduct of sodium fluoride (NaF) with chlorine (Cl2) is not outlined in this chemical equation.

Logically, this reaction would generate Sodium Chloride (2NaCl) and Fluorine gas (F2), as elements tend to react to form stable compounds.

Given this, an error may occur in the original question since the production of Sodium Fluoride (NaF) is not associated with Chlorine gas (Cl2) under normal conditions. The formation of 46.5 g of sodium fluoride does not necessitate the application of chlorine based on the provided reaction.

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How many moles of chlorine are needed to form 46.5 g of sodium fluoride?\[ \text{Reaction: } \text{Cl}_2(l) + 2\text{NaF}(s) \rightarrow \text{F}_2(g) + 2\text{NaCl}(s) \]

Answer :

Final answer:

Explanation:

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Other Questions

How many moles of chlorine are needed to form 46.5 g of sodium fluoride?

\[ \text{Reaction: } \text{Cl}_2(l) + 2\text{NaF}(s) \rightarrow \text{F}_2(g) + 2\text{NaCl}(s) \]