Answer: 34.4 g
Explanation:
[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}[/tex]
[tex]\text{Number of moles of hydrogen}=\frac{5g}{2g/mol}=2.5moles[/tex]
As [tex]CO[/tex] is in excess, [tex]H_2[/tex] is the limiting reagent and thus it will limit the formation of products.
[tex]CO+2H_2\rightarrow CH_3OH[/tex]
According to stoichiometry:
2 moles of hydrogen produce = 1 mole of [tex]CH_3OH[/tex]
2.5 moles of hydrogen produce = [tex]\frac{1}{2}\times 2.5=1.25 moles[/tex] of [tex]CH_3OH[/tex]
Mass of [tex]CH_3OH=moles\times {\text {Molar mass}}=1.25\times 32=40g[/tex]
But as % yield is 86%, mass of [tex]CH_3OH[/tex] produded is [tex]\frac{86}{100}\times 40=34.4g[/tex]
Thus 34.4 g of [tex]CH_3OH[/tex] is produced.
