In the industrial synthesis of acetic acid, methanol is reacted with carbon monoxide. The balanced equation for this reaction is: CH₃OH(g) + CO(g) → CH₃COOH(l)
How many grams of CO(g) are required to produce 16.6 mol of acetic acid?

Question

Quizplus · Accepted Answer

From the balanced equation, we can see that the ratio of CO to acetic acid is 1:1. Therefore, the number of moles of CO required to produce 16.6 mol of acetic acid is also 16.6 mol. 
Using the molar mass of CO (28.01 g/mol), we can calculate the mass of CO required: 
Mass = number of moles x molar mass 
Mass = 16.6 mol x 28.01 g/mol 
Mass = 465 g 
Therefore, the correct answer is C, 465 g.

In the Industrial Synthesis of Acetic Acid, Methanol Is Reacted