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The balanced equation below shows the products that are formed:

[tex]\[ C_5H_{12} + 8O_2 \rightarrow 5CO_2 + 6H_2O \][/tex]


Sagot :

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]