Answer :

Final Answer:

You would get 4.8 grams of water. The limiting reactant is oxygen.

Explanation:

When hydrogen (H₂) and oxygen (O₂) react to form water (H₂O), the balanced chemical equation is:

2H2 + O2 → 2H2O

To calculate the amount of water produced, we need to determine the limiting reactant, which is the reactant that will be completely consumed and determine the amount of product formed.

Calculate the moles of each reactant.

- Moles of hydrogen (H2) = 4.8 g / 2 g/mol = 2.4 moles

- Moles of oxygen (O2) = 38.4 g / 32 g/mol = 1.2 moles

Determine the limiting reactant.

The balanced equation tells us that 2 moles of hydrogen are required for every mole of oxygen. Since we have 2.4 moles of hydrogen and 1.2 moles of oxygen, oxygen is the limiting reactant because it will run out first.

Calculate the moles of water produced.

From the balanced equation, 2 moles of water are formed for every mole of oxygen consumed. Since oxygen is the limiting reactant, we can calculate the moles of water produced as follows:

Moles of water = 1.2 moles of oxygen × 2 moles of water/mole of oxygen = 2.4 moles

Now, we can convert moles to grams:

Mass of water = 2.4 moles × 18 g/mol = 43.2 grams

So, you would get 43.2 grams of water, but you only started with 4.8 grams of hydrogen and 38.4 grams of oxygen. Therefore, the limiting reactant (oxygen) determines the amount of water produced, which is 4.8 grams.

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