if 3.00 moles of water are produced, how many grams of oxygen must be consumed?

I will happily review your thinking or work.

Answered below. You need not repeat duplicate posts.

To determine how many grams of oxygen must be consumed when 3.00 moles of water are produced, you need to use the balanced chemical equation for the reaction in which water is produced.

The balanced chemical equation for the production of water can be written as follows:

2 H₂ + O₂ → 2 H₂O

From the equation, we see that for every 2 moles of water produced, 1 mole of oxygen (O₂) is consumed.

Therefore, to find how many grams of oxygen are needed, we will follow these steps:

Step 1: Convert moles of water to moles of oxygen:
3.00 moles H₂O × (1 mole O₂ / 2 moles H₂O) = 1.50 moles O₂

Step 2: Convert moles of oxygen to grams:
To convert moles of oxygen to grams, we need to know the molar mass of oxygen. The molar mass of oxygen is approximately 32.00 grams/mole.

1.50 moles O₂ × (32.00 grams O₂ / 1 mole O₂) = 48.00 grams O₂

Therefore, when 3.00 moles of water are produced, approximately 48.00 grams of oxygen must be consumed.