Let's break down the equation given and analyze the reaction represented:
The left side of the equation shows the atomic masses of the reactants:
- 24 + 16 = 40 (first reactant)
- 12 + 16 + 16 = 44 (second reactant)
Adding these gives us a total of 40 + 44 = 84.
The right side of the equation indicates the total mass of the products, which is 84.
Now, let's analyze the statements:
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"A molecule with 40 atoms combined with a molecule with 48 atoms to produce a molecule with 84 atoms."
- This is incorrect since the numbers refer to atomic mass, not the number of atoms.
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"A molecule with two atoms combined with a molecule with three atoms to produce a molecule with a mass of 84 u."
- This is incorrect as well; the atomic masses add up to 84 u, but the stated number of atoms (2 and 3) doesn't match the actual masses.
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"Two molecules, each with the same mass, combined to make one molecule."
- This statement is ambiguous. While the total mass is preserved, we don't know if the two molecules have the same mass.
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"Two molecules, each with two atoms, combined to make one molecule."
- This statement is not accurate according to the given atomic masses as the total number of atoms does not add up correctly based on the information provided.
None of the statements accurately represent the reaction as described by the atomic masses in the equation. However, the closest interpretation might be the first statement if we consider it in terms of mass rather than atom count.
None of the options perfectly fit the simplified interpretation of the reaction based on atomic mass alone. If forced to choose the best interpretation, it could be assumed to relate to the transformation of mass rather than a precise count of atoms. Therefore, if you were looking for the most fitting approximation considering atomic mass, that would be the first statement, albeit inaccurately stated.
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