Final answer:
The true statement about heat and/or temperature is that temperature measures the kinetic energy of a substance's molecules. Temperature and kinetic energy are directly related; when kinetic energy increases, the temperature rises, and vice versa.
Step-by-step explanation:
The statement concerning heat and/or temperature that is true is A. Temperature is a measure of the kinetic energy of the molecules of any substance. Temperature is fundamentally a measure of the average kinetic energy of the particles within a substance. When the atoms and molecules in an object are moving or vibrating quickly, they possess higher kinetic energy, and we interpret the object as being "hot". Conversely, when the motion is slow, the kinetic energy is lower, and the object is deemed "cold". This parameter is critical in fields like chemistry, as it influences the rate of chemical reactions and the state changes of matter.
On the contrary, statement B is incorrect because temperature measures kinetic, not potential energy. Lastly, statement C is also incorrect as there is a direct, not inverse, relationship between temperature and heat, assuming no chemical reaction or phase change occurs; increasing the thermal energy will increase the temperature of a substance.