Certainly! Let's analyze the balanced chemical equation to understand the stoichiometric coefficients involved:
[tex]\[
C_5H_{12} + 8 O_2 \rightarrow 5 CO_2 + 6 H_2O
\][/tex]
This equation represents the combustion of pentane (\(C_5H_{12}\)) in the presence of oxygen (\(O_2\)) to produce carbon dioxide (\(CO_2\)) and water (\(H_2O\)).
1. Pentane (\(C_5H_{12}\)) Coefficient:
- In the balanced equation, the coefficient for \(C_5H_{12}\) is 1. This indicates that 1 mole of pentane is involved in the reaction.
2. Oxygen (\(O_2\)) Coefficient:
- The coefficient for \(O_2\) is 8. This means that 8 moles of oxygen are required to completely combust 1 mole of pentane.
3. Carbon Dioxide (\(CO_2\)) Coefficient:
- According to the balanced equation, the coefficient for \(CO_2\) is 5. This shows that 5 moles of carbon dioxide are produced when 1 mole of pentane undergoes complete combustion.
4. Water (\(H_2O\)) Coefficient:
- Finally, the coefficient for \(H_2O\) is 6. This implies that 6 moles of water are generated as a product of the combustion of 1 mole of pentane.
In summary, the balanced chemical equation provides the following stoichiometric coefficients:
- \(1\) mole of \(C_5H_{12}\) (pentane)
- \(8\) moles of \(O_2\) (oxygen)
- \(5\) moles of \(CO_2\) (carbon dioxide)
- \(6\) moles of \(H_2O\) (water)
Hence, the coefficients are:
[tex]\[
(1, 8, 5, 6)
\][/tex]
