A synthesis reaction takes place when carbon monoxide (CO) and hydrogen gas (H2) react to form methanol (CH3OH). How many grams of methanol are produced when 14 grams of carbon monoxide reacts with 1.5 grams of hydrogen gas?

11.92 g ≅ 12.0 g.

Explanation:

The balanced equation of the reaction is: CO + 2H₂ → CH₃OH. The stichiometry shows that 1.0 mole of CO reacts with 2.0 moles of H₂ to produce 1.0 mole of CH₃OH. Now, we need to calculate the no. of moles (n) of the reacted CO and H₂ using the relation: n = mass / molar mass. No. of moles of CO = mass / molar mass = (14.0 g) / (28.01 g/mol) = 0.4999 mol ≅ 0.5 mol. No. of moles of H₂ = mass / molar mass = (1.5 g) / (2.015 g/mol) = 0.7444 mol. As showed in the balanced equation: every 1.0 mole of CO needs 2.0 moles of hydrogen to react completely. So, for the given data H₂ gas (0.7444 mol) will be the limiting reactant that reacts completely with (0.372 mol) of CO which is in excess (0.5 mol). We can get the no. of moles of CH₃OH produced.

Using cross multiplication:

2 moles of H₂ produce → 1.0 mole of CH₃OH, from the stichiometry.

0.7444 moles of H₂ produce →? mole of CH₃OH.

The no. of moles of CH₃OH produced = (0.7444 moles) (1.0 mole) / (2 moles) = 0.372 mol. The amount of CH₃OH produced in grams (mass) = n x molar mass = (0.372 mol) (32.04 g/mol) = 11.92 g ≅ 12.0 g.