Question

Part A - Which numbers are used? Consider the balanced chemical equation that follows. You are asked to determine how many moles of water you can produce from 4.0 molmol 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)2H2(g)+O2(g)→2H2O(l) View Available Hint(s)

Answer 1

Answer: The amount of water formed in the reaction are 4.0 moles

Explanation:

We are given:

Moles of hydrogen gas = 4.0 moles

For the given chemical reaction:

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

By Stoichiometry of the reaction:

2 moles of hydrogen gas produces 2 moles of water.

So, 4.0 moles of hydrogen gas will produce = $\frac{2}{2}\times 4.0=4.0mol$ of water.

Hence, the amount of water formed in the reaction are 4.0 moles