Let's analyze the situation step-by-step:
1. Initial Conditions:
- The ice cube is initially at [tex]\(0^{\circ}C\)[/tex].
- The freezer is at [tex]\(-18^{\circ}C\)[/tex].
2. Thermodynamic Principles:
- According to the second law of thermodynamics, heat transfer occurs from a body at a higher temperature to a body at a lower temperature until thermal equilibrium is reached.
- Since the ice cube is at [tex]\(0^{\circ}C\)[/tex] (which is higher than [tex]\(-18^{\circ}C\)[/tex]), heat will transfer from the ice cube to the colder environment of the freezer.
3. Possible Outcomes:
- Statement A: The ice cube will lose thermal energy to the surroundings.
This is possible because the freezer is at a lower temperature than the ice cube (i.e., [tex]\(-18^{\circ}C\)[/tex] is lower than [tex]\(0^{\circ}C\)[/tex]), so the ice cube would transfer heat to the colder environment.
- Statement B: The ice cube will remain unchanged.
This cannot be true because there will be a temperature difference that will cause the ice to lose thermal energy.
- Statement C: The ice cube will gain mass from the surroundings.
This cannot happen because mass does not spontaneously increase without an external source or other specific conditions being met.
- Statement D: The ice cube will gain thermal energy from the surroundings.
This is not possible because the surroundings (freezer at [tex]\(-18^{\circ}C\)[/tex]) are colder than the ice cube ([tex]\(0^{\circ}C\)[/tex]), making thermal energy transfer to the ice cube impossible under these conditions.
4. Conclusion:
- Considering the principles of heat transfer and the given conditions, the only true statement is:
* Statement A: The ice cube will lose thermal energy to the surroundings.
Thus, the correct answer is:
A. The ice cube will lose thermal energy to the surroundings.
