What defines the relationship between heat (q), mass (m), specific heat capacity (c), and temperature change (ΔT)?

The relationship between heat (q), mass (m), specific heat capacity (c), and temperature change (ΔT) is defined by the equation ( q = mc\Delta T ). This formula represents the amount of heat energy transferred to or from a substance in relation to its mass, the specific heat capacity, and the change in temperature.

In this equation:

• q represents the heat energy (in joules or calories).
• m stands for the mass of the substance (in grams or kilograms).
• c is the specific heat capacity (the amount of heat required to raise the temperature of one gram of the substance by one degree Celsius or one Kelvin).
• ΔT is the change in temperature, calculated as the final temperature minus the initial temperature.

This equation fundamentally conveys that the heat absorbed or released by a substance is directly proportional to its mass and the temperature change, while also depending on the specific heat capacity, which characterizes how much heat a specific material can hold.

The mention of "D" as the answer in your choice signifies the correct representation with the proper symbols and their established relationship, providing clarity in the context of thermodynamic calculations in chemistry.