Question

The products of the combustion of acetone with oxygen are shown in the following equation: __ CH₃coCH₃ __ O₂ → __ CO₂ __ H₂O when properly balanced, the equation indicates that blank 1 mol of O₂ are required for each mole of CH₃coCH₃.

Answer 1

To properly balance the combustion reaction of acetone, 3.5 moles of oxygen (O2) are needed for each mole of acetone (CH3COCH3).

Step-by-step explanation:

To balance the combustion reaction of acetone (CH₃COCH₃) with oxygen (O₂), we need to ensure that the number of atoms of each element is the same on both sides of the equation. Acetone has 3 carbon atoms, 6 hydrogen atoms, and 1 oxygen atom. The products are carbon dioxide (CO₂) and water (H₂O).

Here's the balanced chemical equation for the combustion of acetone:

2 CH₃COCH₃ + 7 O₂ → 6 CO₂ + 6 H₂O

From the equation, we can see that 7 mol of O₂ are required to completely combust 2 mol of acetone. Therefore, for each mole of acetone, 3.5 mol of O₂ are required.