To determine how many moles of hydrogen chloride (HCl) are produced when reacting 2.3 moles of chlorine (Cl[tex]\(_2\)[/tex]) with excess hydrogen (H[tex]\(_2\)[/tex]), we must consider the stoichiometry of the balanced chemical equation:
[tex]\[
H_2 + Cl_2 \rightarrow 2 HCl
\][/tex]
From the balanced equation, we observe that 1 mole of Cl[tex]\(_2\)[/tex] produces 2 moles of HCl. Therefore, the mole ratio of HCl to Cl[tex]\(_2\)[/tex] is:
[tex]\[
\frac{2 \, \text{mol} \, \text{HCl}}{1 \, \text{mol} \, \text{Cl} _2}
\][/tex]
This ratio indicates how many moles of HCl can be formed from a given amount of Cl[tex]\(_2\)[/tex].
So, the correct ratio to use in this case is:
[tex]\[
\frac{2 \, \text{mol} \, \text{HCl}}{1 \, \text{mol} \, \text{Cl} _2}
\][/tex]
Thus, the correct answer is:
C. [tex]\(\frac{2 \, \text{mol} \, \text{HCl}}{1 \, \text{mol} \, \text{Cl} _2}\)[/tex]
