What is the mass of the single product that is formed from the reaction between 2.5 g hydrogen and 7.5 g oxygen?

Question

Quizplus · Accepted Answer

The balanced equation for the reaction between hydrogen and oxygen is:

2H2 + O2 → 2H2O

Therefore, the mole ratio between hydrogen and water is 2:2 or 1:1. This means that all the hydrogen will be used up to form the same amount of water.

To find out the mass of water formed, we need to convert the given masses of hydrogen and oxygen into moles, and then use the mole ratio to determine the amount of water formed. The molar mass of hydrogen is 1.008 g/mol, and the molar mass of oxygen is 15.999 g/mol.

Number of moles of hydrogen = 2.5 g / 1.008 g/mol = 2.48 mol
Number of moles of oxygen = 7.5 g / 15.999 g/mol = 0.469 mol

From the balanced equation, we can see that 2 moles of hydrogen react with 1 mole of oxygen to form 2 moles of water, or 1 mole of hydrogen reacts with 0.5 moles of oxygen to form 1 mole of water.

Since there is not enough oxygen to react with all the hydrogen, oxygen is the limiting reagent in this reaction. This means that only 0.469 moles of water can be formed.

Mass of water formed = number of moles of water x molar mass of water
Mass of water formed = 0.469 mol x 18.015 g/mol = 8.46 g

Therefore, the mass of the single product formed from the reaction between 2.5 g hydrogen and 7.5 g oxygen is 8.46 g, which is closest to answer choice D.

What Is the Mass of the Single Product That Is