Question

The reaction between CO₂ and H₂ produces methanol CH₄O and water? How many grams of methanol are produced when 50 g of CO₂ are mixed with 25 g of H2?

Answer 1

The balanced equation for the reaction between CO₂ and H₂ is CO₂ + 4H₂ → CH₄O + H₂O. Using the balanced equation, we can calculate the grams of CH₄O produced. In this case, 36.36 grams of CH₄O are produced when 50 grams of CO₂ are mixed with 25 grams of H₂.

Step-by-step explanation:

In order to determine the amount of methanol produced, we need to use the stoichiometry of the balanced chemical equation. The balanced equation for the reaction between CO₂ and H₂ is:

CO₂ + 4H₂ → CH₄O + H₂O

From the equation, we can see that for every 1 mole of CO₂, 1 mole of CH₄O is produced. To find the grams of CH₄O produced, we can use the molar mass of CH₄O:

Molar mass of CH₄O = 12.01 g/mol (C) + 1.01 g/mol (H) + 16.00 g/mol (O) = 32.02 g/mol

Now, we can calculate the moles of CH₄O produced:

Moles of CH₄O = (50 g CO₂) * (1 mol CO₂/44.01 g CO₂) * (1 mol CH₄O/1 mol CO₂) = 1.136 mol CH₄O

Finally, we can convert the moles of CH₄O to grams:

Grams of CH₄O = (1.136 mol CH₄O) * (32.02 g/mol CH₄O) = 36.36 g CH₄O