Consider the data for substance X given in Exercise 117 ....

Consider the data for substance $X$ given in Exercise 117 . When the temperature of 1.000 mole of $X(g)$ is lowered from $100.0^{\circ} \mathrm{C}$ to form $\mathrm{X}(l)$ at $50.0^{\circ} \mathrm{C}, 28.75 \mathrm{kJ}$ of heat is released. Calculate the specific heat capacity of $\mathrm{X}(g)$

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Key Concepts

Specific Heat Capacity

Specific heat capacity is the property of a substance that defines the amount of heat needed to raise the temperature of a given amount (per unit mass or per mole) of that substance by one degree Celsius or Kelvin. It is used in calculations involving the thermal energy required or released when a substance undergoes a temperature change without a phase change.

Sensible and Latent Heat

In thermal processes, sensible heat is the heat exchanged that results in a measurable change in temperature, while latent heat is the energy absorbed or released during a phase change at constant temperature. Understanding the difference is critical in processes where both temperature change and phase changes occur, as it determines how to properly partition the total heat transfer.

Calorimetry

Calorimetry is the experimental technique and theoretical framework used to measure the heat exchanged in physical and chemical processes. This involves applying the principles of energy conservation and using relationships such as Q = n·c·?T for calculating the sensible heat change, as well as incorporating latent heat effects when a phase change is involved.

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