Question
The following equation represents the atomic masses of the reactants and products in a chemical reaction.
(24 + 16) + (12 + 16 + 16) = 84
Which statement about the reaction is correct?
(1 point)
Responses
Two molecules, each with two atoms, combined to make one molecule.
Two molecules, each with two atoms, combined to make one molecule.
A molecule with 40 atoms combined with a molecule with 48 atoms to produce a molecule with 84 atoms.
A molecule with 40 atoms combined with a molecule with 48 atoms to produce a molecule with 84 atoms.
A molecule with two atoms combined with a molecule with three atoms to produce a molecule with a mass of 84 u.
A molecule with two atoms combined with a molecule with three atoms to produce a molecule with a mass of 84 u.
Two molecules, each with the same mass, combined to make one molecule.
(24 + 16) + (12 + 16 + 16) = 84
Which statement about the reaction is correct?
(1 point)
Responses
Two molecules, each with two atoms, combined to make one molecule.
Two molecules, each with two atoms, combined to make one molecule.
A molecule with 40 atoms combined with a molecule with 48 atoms to produce a molecule with 84 atoms.
A molecule with 40 atoms combined with a molecule with 48 atoms to produce a molecule with 84 atoms.
A molecule with two atoms combined with a molecule with three atoms to produce a molecule with a mass of 84 u.
A molecule with two atoms combined with a molecule with three atoms to produce a molecule with a mass of 84 u.
Two molecules, each with the same mass, combined to make one molecule.
Answers
GPT-4o mini
To analyze the given equation:
\[
(24 + 16) + (12 + 16 + 16) = 84
\]
We can break it down as follows:
- The left-hand side represents the total mass of the reactants.
- \(24 + 16 = 40\) could represent the mass of one reactant (which may correspond to a molecule).
- \(12 + 16 + 16 = 44\) represents the mass of the second reactant (also possibly a molecule).
- When added together, \(40 + 44 = 84\), which suggests the formation of a product with a mass of 84.
Now, let's evaluate the options provided:
1. **Two molecules, each with two atoms, combined to make one molecule.**
- This is incorrect because the molecular masses suggest larger molecules.
2. **A molecule with 40 atoms combined with a molecule with 48 atoms to produce a molecule with 84 atoms.**
- This is incorrect because the total masses from the equation do not correspond to the number of atoms, as the masses refer to atomic mass units (u) and not the number of atoms directly.
3. **A molecule with two atoms combined with a molecule with three atoms to produce a molecule with a mass of 84 u.**
- This statement is not directly supported since we cannot infer the number of atoms from the atomic masses given.
4. **Two molecules, each with the same mass, combined to make one molecule.**
- This is incorrect since the two mass values are not the same.
None of the statements correctly summarize the reaction based on the data provided. However, the most reasonable interpretation, if we focus strongly on mass, would be along the third option, although not strictly accurate regarding the atom counts.
If only focusing on mass relationships without the complications of atom counting, for simple discussion, it would lean towards reacting smaller masses to give a larger mass without getting caught in atom specifics:
Thus, while more realization is needed to determine atoms, we can summarize:
**Best answer among the options would be:**
**A molecule with two atoms combined with a molecule with three atoms to produce a molecule with a mass of 84 u.** (Not perfect, but closest in logical interpretation on mass).
\[
(24 + 16) + (12 + 16 + 16) = 84
\]
We can break it down as follows:
- The left-hand side represents the total mass of the reactants.
- \(24 + 16 = 40\) could represent the mass of one reactant (which may correspond to a molecule).
- \(12 + 16 + 16 = 44\) represents the mass of the second reactant (also possibly a molecule).
- When added together, \(40 + 44 = 84\), which suggests the formation of a product with a mass of 84.
Now, let's evaluate the options provided:
1. **Two molecules, each with two atoms, combined to make one molecule.**
- This is incorrect because the molecular masses suggest larger molecules.
2. **A molecule with 40 atoms combined with a molecule with 48 atoms to produce a molecule with 84 atoms.**
- This is incorrect because the total masses from the equation do not correspond to the number of atoms, as the masses refer to atomic mass units (u) and not the number of atoms directly.
3. **A molecule with two atoms combined with a molecule with three atoms to produce a molecule with a mass of 84 u.**
- This statement is not directly supported since we cannot infer the number of atoms from the atomic masses given.
4. **Two molecules, each with the same mass, combined to make one molecule.**
- This is incorrect since the two mass values are not the same.
None of the statements correctly summarize the reaction based on the data provided. However, the most reasonable interpretation, if we focus strongly on mass, would be along the third option, although not strictly accurate regarding the atom counts.
If only focusing on mass relationships without the complications of atom counting, for simple discussion, it would lean towards reacting smaller masses to give a larger mass without getting caught in atom specifics:
Thus, while more realization is needed to determine atoms, we can summarize:
**Best answer among the options would be:**
**A molecule with two atoms combined with a molecule with three atoms to produce a molecule with a mass of 84 u.** (Not perfect, but closest in logical interpretation on mass).