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Which of the following chemical equations is balanced?
2H ₂ + O ₂ → 2H ₂ O
H ₂ + 2O ₂ → 2H ₂ O
H ₂ + O ₂ → H ₂ O
H ₂ O + O ₂ → H ₂ O ₂
2H ₂ + O ₂ → 2H ₂ O
A chemical equation is balanced when the number of atoms of each element is equal on both the reactant side and the product side, adhering to the Law of Conservation of Mass. In Option A (2H₂ + O₂ → 2H₂O), both sides contain 4 Hydrogen atoms and 2 Oxygen atoms, making it balanced.
A chemical equation is balanced when the number of atoms of each element is equal on both the reactant side and the product side, adhering to the Law of Conservation of Mass. In Option A (2H₂ + O₂ → 2H₂O), both sides contain 4 Hydrogen atoms and 2 Oxygen atoms, making it balanced.
Law of Conservation of Mass (formulated by Antoine Lavoisier in 1789) states that mass can neither be created nor destroyed in a chemical reaction.
Law of Conservation of Mass dictates that mass is conserved during a chemical transformation.
Stoichiometric coefficients (numbers in front of chemical formulas) are used to balance equations.
Subscripts (numbers within chemical formulas) indicate atom count per molecule and must never be altered when balancing.
Option A is correct because both reactants and products contain 4 H atoms and 2 O atoms.
Option B (H₂ + 2O₂ → 2H₂O) has 2 H and 4 O on the left, but 4 H and 2 O on the right (Unbalanced).
Option C (H₂ + O₂ → H₂O) has 2 O on the left and only 1 O on the right (Unbalanced).
Option D (H₂O + O₂ → H₂O₂) has 3 O on the left and 2 O on the right (Unbalanced).
A is correct — Option A maintains equal numbers of Hydrogen (4) and Oxygen (2) atoms on both reactant and product sides.
Questions on balancing equations are closely linked to chemical stoichiometry and mole concept calculations frequently tested in general science sections.
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