Balance the following equations. (b) P 4 O 10 + H 2 O → H 3 PO 4

Hey everyone. We're asked to balance the following chemical reaction. We can start by counting the number of atoms we have on both sides. Starting off with our calcium in our react inside we have three of calcium, two of nitrogen, two of hydrogen and one of oxygen. Looking at our product side, we have one of calcium, one of nitrogen, five of hydrogen and two of oxygen. We can start off by balancing out our calcium by adding a three prior to our calcium hydroxide. When we do this, we end up with three of calcium, nine of hydrogen and six of oxygen. Looking at our nitrogen, we can balance this out by adding a two prior to our ammonia. When we add this to, we change our nitrogen into two And we also change our hydrogen from a nine into a 12. Now to finish off this question, we can balance off our hydrogen and oxygen by adding a six prior to our water. So we end up with 12 of hydrogen and six of oxygen and this will be our final balanced chemical equation. So I hope this made sense. And let us know if you have any questions

Ch.3 - Mass Relationships in Chemical Reactions

McMurry8th EditionChemistryISBN: 9781292336145Not the one you use?Change textbook

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McMurry 8th Edition

Ch.3 - Mass Relationships in Chemical Reactions

Problem 40b

Chapter 3, Problem 40b

Balance the following equations. (b) P₄O₁₀ + H₂O → H₃PO₄

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Identify the reactants and products in the chemical equation: \( \text{P}_4\text{O}_{10} + \text{H}_2\text{O} \rightarrow \text{H}_3\text{PO}_4 \).

Count the number of each type of atom on both sides of the equation. Initially, there are 4 phosphorus (P) atoms, 10 oxygen (O) atoms, and 2 hydrogen (H) atoms on the reactant side.

On the product side, each \( \text{H}_3\text{PO}_4 \) molecule contains 3 hydrogen (H) atoms, 1 phosphorus (P) atom, and 4 oxygen (O) atoms. Determine how many \( \text{H}_3\text{PO}_4 \) molecules are needed to balance the phosphorus atoms.

Adjust the coefficients of \( \text{H}_2\text{O} \) and \( \text{H}_3\text{PO}_4 \) to balance the hydrogen and oxygen atoms. Remember that the number of each type of atom must be the same on both sides of the equation.

Verify that the equation is balanced by ensuring that the number of each type of atom is equal on both sides. Adjust coefficients as necessary to achieve balance.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Balancing Chemical Equations

Balancing chemical equations involves ensuring that the number of atoms for each element is the same on both sides of the equation. This is based on the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction. Coefficients are used to adjust the quantities of reactants and products to achieve balance.

Molecular Formulas

Molecular formulas represent the actual number of atoms of each element in a molecule. For example, P4O10 indicates that there are four phosphorus atoms and ten oxygen atoms in the compound. Understanding molecular formulas is crucial for identifying the substances involved in a reaction and for determining how they combine or react with one another.

Stoichiometry

Stoichiometry is the quantitative relationship between reactants and products in a chemical reaction. It allows chemists to calculate the amounts of substances consumed and produced in a reaction based on balanced equations. This concept is essential for predicting yields and understanding the proportions in which reactants react to form products.