To determine how many moles of [tex]\( \text{COCl}_2 \)[/tex] will be produced when 0.90 moles of [tex]\( \text{Cl}_2 \)[/tex] react fully with carbon monoxide ([tex]\(CO\)[/tex]), we need to use the balanced chemical equation and the concept of molar ratios.
The balanced chemical equation is:
[tex]\[
CO (g) + Cl_2 (g) \rightarrow COCl_2 (g)
\][/tex]
From the equation, you can see that 1 mole of carbon monoxide ([tex]\(CO\)[/tex]) reacts with 1 mole of chlorine gas ([tex]\(Cl_2\)[/tex]) to produce 1 mole of phosgene ([tex]\(COCl_2\)[/tex]). This indicates a 1:1 molar ratio between chlorine gas ([tex]\(Cl_2\)[/tex]) and phosgene ([tex]\(COCl_2\)[/tex]).
Given that we have 0.90 moles of [tex]\(Cl_2\)[/tex]:
- According to the 1:1 molar ratio, 0.90 moles of [tex]\(Cl_2\)[/tex] will produce the same amount of [tex]\(COCl_2\)[/tex].
Therefore:
[tex]\[
0.90 \text{ moles of } Cl_2 \text{ will produce } 0.90 \text{ moles of } COCl_2.
\][/tex]
Hence, the correct answer is:
[tex]\[
0.90 \text{ moles of } COCl_2.
\][/tex]
