Which of the following statements is true for the reaction N_2(g) + 3 H_2(g) → 2 NH_3(g)?

• A. The reaction is not balanced because there are more nitrogen atoms on the product side.
• B. The reaction is balanced because the number of atoms of each element is the same on both sides.
• C. The reaction is not balanced because the number of molecules is not the same on both sides.
• D. The reaction is not balanced because there are more hydrogen atoms on the reactant side.

Answer: (B)

Verified step by step guidance

1. Identify the chemical equation given: \(\mathrm{N_2(g) + 3\ H_2(g) \rightarrow 2\ NH_3(g)}\).
2. Count the number of nitrogen atoms on both sides: On the reactant side, there are 2 nitrogen atoms in \(\mathrm{N_2}\); on the product side, there are 2 molecules of \(\mathrm{NH_3}\), each containing 1 nitrogen atom, so total nitrogen atoms = 2.
3. Count the number of hydrogen atoms on both sides: On the reactant side, there are 3 molecules of \(\mathrm{H_2}\), each with 2 hydrogen atoms, so total hydrogen atoms = 6; on the product side, there are 2 molecules of \(\mathrm{NH_3}\), each with 3 hydrogen atoms, so total hydrogen atoms = 6.
4. Compare the number of atoms of each element on both sides to check if they are equal. If they are equal, the reaction is balanced in terms of atoms.
5. Note that balancing a chemical equation requires equal numbers of each type of atom on both sides, not necessarily the same number of molecules. Therefore, the correct statement is that the reaction is balanced because the number of atoms of each element is the same on both sides.