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? 2H2(g)+O2(g)→2H2O(l)

Answer 1

4 mol H2 (2 mol H2O / 2 mol H2) gives a theoretical yield of 4 moles of H2O. You use the 2 mol H2 per 2 mol H2O to perform this calculation hope this helps

Answer 2

Answer: 4 moles of water are produced.

Number 2 is used to perform this calculation

Step-by-step explanation:

The balanced chemical equation is:

`2H_2(g)+O_2(g)\rightarrow 2H_2O(l)`

As it is given, excess oxygen is present, oxygen acts as excess reagent and hydrogen acts as limiting reagent as it limits the formation of products

According to stoichiometry:

2 moles of hydrogen give = 2 moles of water

Thus 4 moles of hydrogen give =
`(2)/(2)* 4=4` moles of water

4 moles of water are produced . Thus the coefficient 2 from hydrogen and coefficient 2 from water that appear in the balanced chemical equation is used.