To determine how much sodium chloride ([tex]\( \text{NaCl} \)[/tex]) could be formed when [tex]\( 2.5 \, \text{mol} \, \text{Na} \)[/tex] and [tex]\( 1.1 \, \text{mol} \, \text{Cl}_2 \)[/tex] are placed in a flask and allowed to react, we start by examining the reaction stoichiometry given by the balanced chemical equation:
[tex]\[ 2 \, \text{Na} + \text{Cl}_2 \rightarrow 2 \, \text{NaCl} \][/tex]
This equation tells us that 2 moles of sodium (Na) react with 1 mole of chlorine gas ([tex]\( \text{Cl}_2 \)[/tex]) to produce 2 moles of sodium chloride ([tex]\( \text{NaCl} \)[/tex]).
### Step 1: Identify the Limiting Reactant
- Since 2 moles of Na react with 1 mole of [tex]\( \text{Cl}_2 \)[/tex], the mole ratio of Na to [tex]\( \text{Cl}_2 \)[/tex] is 2:1.
Let's determine how many moles of [tex]\( \text{NaCl} \)[/tex] can be formed by each reactant separately:
1. Sodium (Na):
- We have 2.5 moles of Na.
- According to the stoichiometry, 2 moles of Na produce 2 moles of [tex]\( \text{NaCl} \)[/tex].
- Therefore, [tex]\( 2.5 \)[/tex] moles of Na would produce [tex]\( 2.5 \)[/tex] moles of [tex]\( \text{NaCl} \)[/tex],
assuming there is enough [tex]\( \text{Cl}_2 \)[/tex].
2. Chlorine gas ([tex]\( \text{Cl}_2 \)[/tex]):
- We have 1.1 moles of [tex]\( \text{Cl}_2 \)[/tex].
- According to the stoichiometry, 1 mole of [tex]\( \text{Cl}_2 \)[/tex] produces 2 moles of [tex]\( \text{NaCl} \)[/tex].
- Therefore, [tex]\( 1.1 \)[/tex] moles of [tex]\( \text{Cl}_2 \)[/tex] would produce [tex]\( 2 \times 1.1 = 2.2 \)[/tex] moles of [tex]\( \text{NaCl} \)[/tex],
assuming there is enough Na.
### Step 2: Determine the Amount of NaCl Formed by the Limiting Reactant
- The reactant that produces fewer moles of [tex]\( \text{NaCl} \)[/tex] is the limiting reactant.
- Since chlorine gas ([tex]\( \text{Cl}_2 \)[/tex]) produces only [tex]\( 2.2 \)[/tex] moles of [tex]\( \text{NaCl} \)[/tex] and still follows the stoichiometric ratio, [tex]\( \text{Cl}_2 \)[/tex] is the limiting reactant.
Hence, the amount of [tex]\( \text{NaCl} \)[/tex] that could be formed is determined by the limiting reactant, which is chlorine gas ([tex]\( \text{Cl}_2 \)[/tex]) in this case.
### Conclusion
- The maximum amount of sodium chloride ([tex]\( \text{NaCl} \)[/tex]) that can be formed is [tex]\( 2.2 \)[/tex] moles.
Thus, the correct answer is:
C. 2.2 mol, because the amount of product is determined by the limiting reactant, chlorine.
