Chemical reaction stoichiometry: Calculating moles of hydrogen produced

How many moles of hydrogen are produced when 6.28 mol of oxygen form?

a. 3.14 mol

b. 6.28 mol

c. 12.6 mol

d. 25.2 mol

Final answer:

When 6.28 mol of oxygen form water through the reaction with hydrogen, the stoichiometry of the balanced equation (2H2 + O2 -> 2H2O) indicates that 12.56 mol of hydrogen are produced, which rounds to 12.6 mol, answering the student's question with option c.

Explanation: The question regards the amount of hydrogen produced from the reaction of oxygen, which is a basic stoichiometric calculation in chemistry. Balancing the chemical equation for the formation of water from hydrogen and oxygen, we have 2H2 + O2 → 2H2O. The balanced equation indicates that two moles of hydrogen react with one mole of oxygen to produce two moles of water. Therefore, for every mole of oxygen, two moles of hydrogen are required for the reaction.

In the given scenario, 6.28 moles of oxygen are reacting, hence:

(6.28 mol O2) x (2 mol H2 / 1 mol O2) = 12.56 mol H2

According to stoichiometric principles, 12.56 moles of hydrogen would be produced when 6.28 moles of oxygen are used in the reaction. This leads us to the correct answer, which is c. 12.6 mol of hydrogen (rounded to three significant figures).