Question

Consider the balanced chemical equation that follows. You are asked to determine how many moles of water you can produce from 4.0 mol of hydrogen and excess oxygen. (Excess oxygen means that so much oxygen is available it will not run out.) Which of the numbers that appear in the balanced chemical equation below are used to perform this calculation?

Answer 1

Explanation:

According to law of conservation of mass, mass of the reactants is equal to the mass of products in a chemical equation. As mass can neither be created nor it can be destroyed but it can be transformed from one form to another.

As it is given that hydrogen and in excess oxygen is reacting that leads to the formation of water. Hence, the chemical reaction equation will be as follows.

           $2H_{2}(g) + O_{2}(g) \rightarrow 2H_{2}O(l)$

Since, it is given that 4 mol of hydrogen is reacting with excess of oxygen and gives 2 moles of water.

Hence, number of moles of water produced is calculated as follows.

              4 mol of $H_{2} \times \frac{2 mol of H_{2}O}{2 mol of H_{2}}$

                  = 4 moles of $H_{2}O$

Thus, we can conclude that 4 moles of water you can produce from 4.0 mol of hydrogen and excess oxygen.