When the following chemical equation is balanced, what are the correct coefficients for Sb, O_2, and Sb_4O_6?__ Sb + __ O_2 → __ Sb_4O_6

• A. 8 Sb + 6 O_2 → 2 Sb_4O_6
• B. 2 Sb + 3 O_2 → 1 Sb_4O_6
• C. 4 Sb + 3 O_2 → 1 Sb_4O_6
• D. 1 Sb + 2 O_2 → 1 Sb_4O_6

Answer: (C)

Verified step by step guidance

1. Identify the chemical species involved in the reaction: antimony (Sb), oxygen (O_2), and antimony oxide (Sb_4O_6). The goal is to balance the equation so that the number of atoms of each element is the same on both sides.
2. Write the unbalanced equation with coefficients as variables: \(a \, Sb + b \ O_2 \rightarrow c \ Sb_4O_6\).
3. Balance the antimony (Sb) atoms first. Since each molecule of \(Sb_4O_6\) contains 4 Sb atoms, the total Sb atoms on the product side is \$4c\(. Therefore, set \)a = 4c$ to balance Sb atoms.
4. Balance the oxygen (O) atoms next. Each \(O_2\) molecule has 2 oxygen atoms, and each \(Sb_4O_6\) molecule has 6 oxygen atoms. So, the total oxygen atoms on the reactant side is \$2b\(, and on the product side is \)6c\(. Set \)2b = 6c$ to balance oxygen atoms.
5. Choose the smallest whole number value for \(c\) (usually 1) and solve for \(a\) and \(b\) using the relationships \(a = 4c\) and \$2b = 6c$. This will give the balanced coefficients for Sb, O_2, and Sb_4O_6.