Calculating the Number of Moles of Hydrogen and Oxygen

Oct 13, 2025 by pynkocean.com 43 views

Understanding the Chemical Reaction

The chemical reaction between hydrogen and oxygen to form water is a fundamental concept in chemistry. The reaction is as follows:

2H2 + O2 → 2H2O

In this reaction, 2 moles of hydrogen gas (H2) react with 1 mole of oxygen gas (O2) to produce 2 moles of water (H2O). The question asks us to calculate the mass of water produced when 10 grams of hydrogen combine with 80 grams of oxygen.

Calculating the Number of Moles of Hydrogen and Oxygen

To solve this problem, we need to calculate the number of moles of hydrogen and oxygen present in the given masses. The atomic masses of hydrogen and oxygen are 1 g/mol and 16 g/mol, respectively.

Moles of hydrogen = mass of hydrogen / atomic mass of hydrogen = 10 g / 1 g/mol = 10 mol

Moles of oxygen = mass of oxygen / atomic mass of oxygen = 80 g / 16 g/mol = 5 mol

Determining the Limiting Reactant

From the balanced chemical equation, we can see that 2 moles of hydrogen react with 1 mole of oxygen. Therefore, the mole ratio of hydrogen to oxygen is 2:1. We can calculate the number of moles of hydrogen required to react with 5 moles of oxygen as follows:

Moles of hydrogen required = 2 x moles of oxygen = 2 x 5 mol = 10 mol

Since we have 10 moles of hydrogen available, which is equal to the number of moles required, both hydrogen and oxygen are present in excess. Therefore, the reaction will proceed until one of the reactants is completely consumed.

Calculating the Mass of Water Produced

Since both hydrogen and oxygen are present in excess, the reaction will proceed until 5 moles of oxygen are completely consumed. From the balanced chemical equation, we can see that 2 moles of water are produced for every 1 mole of oxygen consumed. Therefore, the number of moles of water produced is:

Moles of water produced = 2 x moles of oxygen consumed = 2 x 5 mol = 10 mol

The mass of water produced can be calculated as follows:

Mass of water produced = moles of water produced x molar mass of water = 10 mol x 18 g/mol = 180 g

However, this is not the correct answer. We need to consider the fact that the reaction is not 100% efficient, and some of the reactants may not be converted to products. In this case, we can assume that the reaction is 100% efficient, and all of the reactants are converted to products.

Calculating the Mass of Water Produced (Corrected)

Since the reaction is 100% efficient, the mass of water produced can be calculated as follows:

Mass of water produced = (moles of hydrogen x molar mass of water) + (moles of oxygen x molar mass of water) = (10 mol x 18 g/mol) + (5 mol x 18 g/mol) = 180 g + 90 g = 270 g

However, this is still not the correct answer. We need to consider the fact that the question asks us to calculate the mass of water produced when 10 grams of hydrogen combine with 80 grams of oxygen. We can calculate the mass of water produced as follows:

Mass of water produced = (mass of hydrogen x molar mass of water) / (molar mass of hydrogen x 2) + (mass of oxygen x molar mass of water) / (molar mass of oxygen x 1) = (10 g x 18 g/mol) / (1 g/mol x 2) + (80 g x 18 g/mol) / (16 g/mol x 1) = 90 g + 90 g = 180 g

Mass of water produced = (mass of hydrogen x molar mass of water) / (molar mass of hydrogen x 2) + (mass of oxygen x molar mass of water) / (molar mass of oxygen x 1) = (10 g x 18 g/mol) / (

Understanding the Chemical Reaction

The chemical reaction between hydrogen and oxygen to form water is a fundamental concept in chemistry. The reaction is as follows:

2H2 + O2 → 2H2O

Calculating the Number of Moles of Hydrogen and Oxygen

To solve this problem, we need to calculate the number of moles of hydrogen and oxygen present in the given masses. The atomic masses of hydrogen and oxygen are 1 g/mol and 16 g/mol, respectively.

Moles of hydrogen = mass of hydrogen / atomic mass of hydrogen = 10 g / 1 g/mol = 10 mol

Moles of oxygen = mass of oxygen / atomic mass of oxygen = 80 g / 16 g/mol = 5 mol

Determining the Limiting Reactant

Moles of hydrogen required = 2 x moles of oxygen = 2 x 5 mol = 10 mol

Calculating the Mass of Water Produced

Moles of water produced = 2 x moles of oxygen consumed = 2 x 5 mol = 10 mol

The mass of water produced can be calculated as follows:

Mass of water produced = moles of water produced x molar mass of water = 10 mol x 18 g/mol = 180 g

Calculating the Mass of Water Produced (Corrected)

Since the reaction is 100% efficient, the mass of water produced can be calculated as follows:

Mass of water produced = (moles of hydrogen x molar mass of water) / (molar mass of hydrogen x 2) + (moles of oxygen x molar mass of water) / (molar mass of oxygen x 1) = (10 g x 18 g/mol) / (1 g/mol x 2) + (80 g x 18 g/mol) / (16 g/mol x 1) = 90 g + 90 g = 180 g

Mass of water produced = (mass of hydrogen x molar mass of water) / (molar mass of