The question asks about a fundamental concept in thermodynamics: the amount of energy needed to change the temperature of a specific quantity of a substance. Understanding this concept is crucial for studying how different materials absorb or release heat energy.

Energy and Specific Heat Capacity Explained

The energy required to raise the temperature of a substance is a key thermal property of that material. When we specify a mass of 1 kg and a temperature change of 1°C (or 1 Kelvin, as the magnitude of the change is the same), we are defining a very specific thermal property of the substance.

Let's analyze the given options in the context of the question:

• Specific Heat Capacity: This term precisely defines the energy required to raise the temperature of a unit mass (typically 1 kg) of a substance by one degree Celsius (or Kelvin). It is an intrinsic material property and is commonly denoted by the symbol \(c\). The formula for heat transfer (\(Q\)) related to temperature change is given by:

  \(Q = mc\Delta T\)

  Where:

  • \(Q\) is the heat energy transferred (measured in Joules, J)
  • \(m\) is the mass of the substance (measured in kilograms, kg)
  • \(c\) is the specific heat capacity of the substance (measured in J/kg·°C or J/kg·K)
  • \(\Delta T\) is the change in temperature (measured in °C or K)

  If we set the mass \(m = 1 \text{ kg}\) and the change in temperature \(\Delta T = 1^\circ\text{C}\), then the equation simplifies to \(Q = c\). This means the heat energy required under these specific conditions is numerically equal to the specific heat capacity of the substance.

• Sensible Heat: This refers to the heat energy that, when added to or removed from a substance, causes a change in its temperature without changing its phase (e.g., solid to liquid or liquid to gas). The energy mentioned in the question (energy causing a temperature rise) is a type of sensible heat, but "specific heat capacity" is the specific property or measure that quantifies this energy for a unit mass and unit temperature change.
• Latent Heat: This is the heat energy absorbed or released by a substance during a phase change (e.g., melting, boiling, condensation, freezing) at a constant temperature. Unlike sensible heat, latent heat does not cause a temperature change. For example, latent heat of fusion is the energy needed to melt ice into water at 0°C, and latent heat of vaporization is for boiling water into steam at 100°C.
• Specific Entropy: Entropy is a thermodynamic property that represents the degree of randomness or disorder within a system. Specific entropy refers to entropy per unit mass. While it is a crucial thermodynamic concept, it does not directly describe the amount of energy needed to raise the temperature of a substance by a specific amount.

Understanding Heat Transfer Concepts

The question precisely defines the specific heat capacity. It quantifies how much energy is needed to heat up a particular material by a standard amount. Different materials possess varying specific heat capacities; for instance, water has a significantly higher specific heat capacity compared to many metals. This means water requires a greater amount of energy to raise its temperature by the same degree.

Therefore, the amount of energy required to raise the temperature of a substance of 1 kg mass by 1°C is accurately defined as its specific heat capacity.