what theoretical yield of formaldehyde (in grams) is expected from the reaction of 44.3 g of methanol? (Assume that methanol is the limiting reactant.)
Look at my response to a stoichiometric problem one question below by Kyle. Post any specific questions after you have studied this procedure and give details about what you don't understand.
To determine the theoretical yield of formaldehyde from the reaction of methanol, you need to follow these steps:
Step 1: Write the balanced chemical equation for the reaction. The balanced equation for the reaction of methanol (CH3OH) to form formaldehyde (CH2O) is:
CH3OH(l) → CH2O(g) + H2(g)
Step 2: Calculate the molar mass of methanol and formaldehyde.
The molar mass of methanol (CH3OH) is:
(1 * 1.01 g/mol) + (4 * 1.01 g/mol) + 16.00 g/mol = 32.04 g/mol
The molar mass of formaldehyde (CH2O) is:
(1 * 12.01 g/mol) + (2 * 1.01 g/mol) + 16.00 g/mol = 30.03 g/mol
Step 3: Determine the limiting reactant.
To determine the limiting reactant, you need to compare the moles of methanol to moles of formaldehyde using the stoichiometry of the balanced equation. The stoichiometric ratio between methanol and formaldehyde is 1:1.
44.3 g of methanol can be converted to moles using its molar mass:
44.3 g / 32.04 g/mol = 1.38 mol
Since the stoichiometric ratio is 1:1, the number of moles of formaldehyde produced will also be 1.38 mol.
Step 4: Calculate the theoretical yield of formaldehyde in grams.
To calculate the theoretical yield, multiply the number of moles of formaldehyde by its molar mass:
1.38 mol * 30.03 g/mol = 41.4 g
Therefore, the theoretical yield of formaldehyde from the reaction of 44.3 g of methanol is expected to be 41.4 grams.