Answer :
Final answer:
In this chemical reaction, the limiting reactant is oxygen. The reaction of 4.8 g of hydrogen with 38.4 g of oxygen would result in the formation of 43.24 g of water.
Explanation:
In order to determine how much water would form when hydrogen reacts with oxygen, we need to use the concept of stoichiometry. The balanced chemical equation for the reaction is 2H2 + O2 → 2H2O.
First, we need to convert the given masses of hydrogen and oxygen to moles using their molar masses, which are 2.02 g/mol for hydrogen and 32.00 g/mol for oxygen. Dividing the given masses by the molar masses, we find that there are 2.376 moles of hydrogen and 1.20 moles of oxygen.
From the balanced equation, we can see that 2 moles of hydrogen react with 1 mole of oxygen to form 2 moles of water. Therefore, the limiting reactant is oxygen, since we have less moles of oxygen compared to hydrogen. Using the mole ratio, we can calculate the moles of water formed, which is 2.40 moles. Finally, we convert moles of water to grams using its molar mass of 18.02 g/mol, giving us 43.24 g of water.
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