To determine which statement best describes the mass of gold and iron atoms based on their specific heat values, we begin by understanding the concept of specific heat. Specific heat is the amount of heat energy required to raise the temperature of one gram of a substance by one degree Celsius.
Given the specific heat values:
- Gold: 0.129 joules/gram °C
- Iron: 0.450 joules/gram °C
Step-by-step explanation:
1. Specific Heat and Density/Mass Relationship:
- A substance with a lower specific heat will heat up faster than a substance with a higher specific heat when the same amount of energy is applied. This indicates that the substance with the lower specific heat requires less energy to increase the temperature of each gram, which typically implies that the atoms of the substance are heavier or denser because it stores less heat per unit mass.
- Conversely, a substance with a higher specific heat will heat up more slowly since more energy is needed to raise the temperature of each gram, suggesting that the atoms are lighter or less dense.
2. Comparing Specific Heat Values:
- Gold has a specific heat of 0.129 joules/gram °C, which is lower than that of iron, having a specific heat of 0.450 joules/gram °C.
- Since gold requires less energy per gram to heat up, it indicates that gold atoms are “heavier” in terms of atomic mass than iron atoms.
3. Conclusion:
- The specific heat values suggest that gold atoms are heavier than iron atoms.
Therefore, the statement that best describes the mass of gold and iron atoms based on their respective specific heat values is:
Gold atoms are heavier than iron atoms.
Thus, the correct statement is:
[tex]$\boxtimes$[/tex] Gold atoms are heavier than iron atoms.
