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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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.

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01:32

Balancing Chemical Equations

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.

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02:08

Determining Molecular Formulas

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.

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