To determine which statement is true about the given reaction, we need to examine the balanced equation and the stoichiometry of the reaction.
The balanced equation is:
C₂H₁₂ (1) + 80₂(g) → 5CO₂(g) + 6H₂O(g)
From the balanced equation, we can see that 1 mole of C₂H₁₂ reacts with 80₂ to produce 5 moles of CO₂ and 6 moles of H₂O.
Now let's analyze the statements:
1. 9 grams of reactants chemically change into 11 grams of product: This statement cannot be determined from the given information because we don't know the molar masses of the substances involved.
2. 9 atoms of reactants chemically change into 11 atoms of product: This statement is not true. In a chemical reaction, atoms are neither created nor destroyed. The number of atoms of each element must be conserved. Therefore, the number of atoms of reactants must be equal to the number of atoms of products.
3. 9 moles of reactants chemically change into 11 moles of product: This statement is not true. According to the balanced equation, 1 mole of C₂H₁₂ reacts to produce 5 moles of CO₂ and 6 moles of H₂O, not 11 moles.
4. 9 liters of reactants chemically change into 11 liters of product: This statement cannot be determined without additional information. The volume of a gas depends on various factors such as pressure and temperature. The given equation does not provide enough information to determine the volume ratio.
Therefore, none of the statements provided is true based solely on the given information.