Final answer:
The statement 'Water evaporation is spontaneous and endothermic' is true. Water evaporation is a process that occurs naturally and absorbs heat from its surroundings, hence it's both spontaneous and endothermic.
Step-by-step explanation:
The statement 'Water evaporation is spontaneous and endothermic' is true. The process of water evaporation is indeed endothermic as it requires heat or energy from the surroundings to transform water from its liquid state to gas (steam). This process is referred to as spontaneous because it naturally occurs without the need for any external force or energy input apart from the required heat.
Spontaneous in the context of this statement refers to a process that can proceed without any outside help under given conditions, typically at room temperature. Understand that this does not mean that spontaneous reactions occur instantly but rather they are capable of taking place by themselves under the given conditions.
In the context of thermochemistry, a process is endothermic if it absorbs heat from the surroundings. This is true in the case of water evaporation where heat is extracted from the surroundings, and it's this extracted heat that provides the energy necessary to break the intermolecular forces of attraction between water molecules, enabling evaporation to occur.
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