The question seems to be about the amount of carbon monoxide required for the production of acetic acid from methanol, but mistakenly refers to carbon dioxide. Correct stoichiometry and reaction conditions are needed to calculate the mass of carbon monoxide required using the mass of methanol provided. The balanced equation involves a 1:1 molar ratio of methanol to carbon monoxide.
The student is asking about the mass of carbon monoxide required to produce acetic acid from methanol. However, there is a mistake in the question; they mentioned carbon dioxide instead of carbon monoxide. To clarify, acetic acid production involving methanol utilizes carbon monoxide, not carbon dioxide. Since the student has provided the mass of methanol but not the reaction equation, we cannot proceed with the calculation without the correct chemical reaction or stoichiometry information. The typical reaction to produce acetic acid from methanol and carbon monoxide is known as the Monsanto process, which can be represented as:
CH3OH(l) + CO(g) → CH3COOH(l)
Both reactants have a 1:1 molar ratio in the balanced equation. To find the mass of carbon monoxide needed, we must first calculate the moles of methanol using its molar mass. Then, since the mole ratio is 1:1, we use the same number of moles to determine the mass of carbon monoxide by multiplying it with its molar mass.
Without further details of the reaction conditions and the assumption that it goes to completion with carbon monoxide in excess, an accurate calculation cannot be performed.