how many grams of water are produced when 2.50 moles of oxygen are used?

Same procedure as below.

90

To determine the number of grams of water produced when 2.50 moles of oxygen (O2) are used, we need to follow these steps:

Step 1: Identify the balanced chemical equation for the reaction that produces water. In this case, it is:

2 H2 + O2 → 2 H2O

This equation tells us that for every 1 mole of O2 consumed, 2 moles of H2O are produced.

Step 2: Calculate the molar mass of water. The molar mass of water (H2O) can be found by adding the molar masses of its components (2 hydrogen atoms and 1 oxygen atom).

Molar mass of H2O = (2 * atomic mass of hydrogen) + atomic mass of oxygen

The atomic mass of hydrogen is approximately 1 gram/mol, and the atomic mass of oxygen is approximately 16 grams/mol.

Molar mass of H2O = (2 * 1 g/mol) + 16 g/mol = 18 g/mol

Step 3: Use the mole ratio from the balanced chemical equation to convert moles of oxygen to moles of water. Since the mole ratio is 1:2 (1 mole of O2 produces 2 moles of H2O), we can use this conversion factor:

2.50 moles O2 * (2 moles H2O/1 mole O2) = 5 moles H2O

Step 4: Convert moles of water to grams of water by multiplying the number of moles by the molar mass of water:

5 moles H2O * 18 g/mol = 90 grams of water

Therefore, when 2.50 moles of oxygen are consumed, 90 grams of water are produced.