Answer :
To determine how many moles of silver chloride ([tex]\( \text{AgCl} \)[/tex]) are produced from 15.0 moles of silver nitrate ([tex]\( \text{AgNO}_3 \)[/tex]), we need to analyze the balanced chemical equation:
[tex]\[ \text{AgNO}_3 + \text{NaCl} \rightarrow \text{NaNO}_3 + \text{AgCl} \][/tex]
From the balanced equation, we see that the reaction is a 1:1 stoichiometric ratio between silver nitrate ([tex]\( \text{AgNO}_3 \)[/tex]) and silver chloride ([tex]\( \text{AgCl} \)[/tex]). This means:
1. For every 1 mole of [tex]\( \text{AgNO}_3 \)[/tex] reacting, 1 mole of [tex]\( \text{AgCl} \)[/tex] is produced.
Given that we have 15.0 moles of [tex]\( \text{AgNO}_3 \)[/tex]:
- The number of moles of [tex]\( \text{AgCl} \)[/tex] produced will be the same as the number of moles of [tex]\( \text{AgNO}_3 \)[/tex] used.
Therefore, from 15.0 moles of silver nitrate, we will produce 15.0 moles of silver chloride.
Hence, the answer is [tex]\( 15.0 \)[/tex] moles.
[tex]\[ \text{AgNO}_3 + \text{NaCl} \rightarrow \text{NaNO}_3 + \text{AgCl} \][/tex]
From the balanced equation, we see that the reaction is a 1:1 stoichiometric ratio between silver nitrate ([tex]\( \text{AgNO}_3 \)[/tex]) and silver chloride ([tex]\( \text{AgCl} \)[/tex]). This means:
1. For every 1 mole of [tex]\( \text{AgNO}_3 \)[/tex] reacting, 1 mole of [tex]\( \text{AgCl} \)[/tex] is produced.
Given that we have 15.0 moles of [tex]\( \text{AgNO}_3 \)[/tex]:
- The number of moles of [tex]\( \text{AgCl} \)[/tex] produced will be the same as the number of moles of [tex]\( \text{AgNO}_3 \)[/tex] used.
Therefore, from 15.0 moles of silver nitrate, we will produce 15.0 moles of silver chloride.
Hence, the answer is [tex]\( 15.0 \)[/tex] moles.
