Answer:
False
Explanation:
When a gas transitions directly to a solid, as in the case of deposition, it is referred to as an endothermic process. This means that energy is required for the transition to occur. In contrast, an exothermic process would release energy into the surroundings.
Let's consider the example of deposition, where gas molecules directly transform into a solid state without passing through the liquid phase. During this transition, the gas molecules slow down and come together to form a solid without the intermediate step of becoming a liquid.
The endothermic nature of this process stems from the fact that energy needs to be absorbed to break the intermolecular forces within the gas molecules and enable them to reorganize into a solid structure. Essentially, this energy is derived from the surroundings, resulting in a decrease in the surrounding temperature.
Therefore, when you encounter the statement "converting a gas to a solid is usually an endothermic process," it signifies that this transition typically necessitates an input of energy from the surroundings to occur.
Hope this helps!