Which statement about heat is true?

The statement that heat will be transferred to the cooler object if there is a temperature difference is a fundamental principle of thermodynamics. This process follows the second law of thermodynamics, which states that heat naturally flows from a region of higher temperature to a region of lower temperature until thermal equilibrium is reached. This means that if you have two objects at different temperatures, energy in the form of heat will move from the hotter object to the cooler one.

This principle is observable in everyday life; for instance, when a hot cup of coffee cools down when left in a cooler environment, the heat energy moves from the coffee into the surrounding air, which is at a lower temperature.

The other statements do not hold universally true. The first statement incorrectly suggests that heat can move from cold to hot spontaneously, which contradicts the second law of thermodynamics. The second statement regarding specific heat being the same for every substance is also incorrect, as specific heat is unique to each substance and is dependent on molecular structure and phase. Lastly, the fourth statement incorrectly implies that specific heat capacity is consistent across all states of matter; however, a substance's specific heat can vary depending on whether it is solid, liquid, or gas due to differences in particle arrangement and energy transfer