Methanol reacts with carbon monoxide in the presence of a catalyst to produce ethanoic acid. Reacted completely with carbon monoxide in a reaction vessel. What is the theoretic yield of ethanioc acid?
Calculate the theoretical yield (in grams of acetic acid, FW 60.05 g/mol) if 8.79 mL of acetic anhydride (FW 102.09 g/mol, density 1.08 g/mL) is used.
To determine the theoretical yield of ethanoic acid, we need to obtain the balanced chemical equation for the reaction between methanol and carbon monoxide.
The balanced chemical equation for the reaction is:
2 CH3OH + CO → CH3COOH
According to the stoichiometry of the balanced equation, we can see that 2 moles of methanol (CH3OH) react with 1 mole of carbon monoxide (CO) to produce 1 mole of ethanoic acid (CH3COOH).
To find the theoretical yield, we need to know the amount of methanol reacted completely. Let's assume you have "x" moles of methanol.
From the balanced equation, it is clear that the reaction produces an equal number of moles of ethanoic acid as there were moles of methanol used. Therefore, the theoretical yield of ethanoic acid will also be "x" moles.
Remember, the theoretical yield represents the maximum amount of product that can be obtained under ideal conditions and assuming 100% conversion of reactants. In practice, actual yield may be lower due to various factors like incomplete reactions or side reactions.