A synthesis reaction takes place when carbon monoxide (CO) and hydrogen gas (H2) react to form methanol (CH3OH). How many grams of methanol

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.

1.solid

2.carbon dioxide

3.helium

2b2t

explanation:

2b2t