In the industrial synthesis of acetic acid, methanol is made to react with carbon monoxide. The balanced equation for this reaction is as follows: 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 mole ratio between CO and acetic acid is 1:1. Therefore, to produce 16.6 mol of acetic acid, we would need 16.6 mol of CO(g).

To convert this to grams, we need to use the molar mass of CO:

1 mol CO(g) = 28.01 g

So,

16.6 mol CO(g) x 28.01 g/mol = 465 g

Therefore, the answer is C) 465 g.

In the Industrial Synthesis of Acetic Acid, Methanol Is Made