Calculate the final temperature that results when (a) a 12.6...

Calculate the final temperature that results when (a) a 12.6 g sample of water at $22.9^{\circ} \mathrm{C}$ absorbs $875 \mathrm{J}$ of heat; (b) a 1.59 kg sample of platinum at $78.2^{\circ} \mathrm{C}$ gives off $1.05 \mathrm{kcal}$ of heat $\left(c_{p}=0.032 \mathrm{cal} \mathrm{g}^{-1} \mathrm{C}^{-1}\right)$

Calculate the final temperature that results when (a) a
12.6 g sample of water at $22.9^{\circ} \mathrm{C}$ absorbs $875 \mathrm{J}$ of heat;
(b) a 1.59 kg sample of platinum at $78.2^{\circ} \mathrm{C}$ gives off $1.05 \mathrm{kcal}$ of heat $\left(c_{p}=0.032 \mathrm{cal} \mathrm{g}^{-1} \mathrm{C}^{-1}\right)$

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Key Concepts

Calorimetry

Calorimetry is the experimental technique used to measure the amount of heat transferred in a chemical or physical process. It involves calculations based on the specific heat capacity and mass of substances to determine the resultant temperature change from the heat gained or lost.

Unit Conversion

In thermal calculations, it is often necessary to convert between different units of energy (such as joules and calories) to maintain consistency in the formulas used. Accurate unit conversion is essential for ensuring that the calculated temperature change is correct.

Specific Heat Capacity

This is the property of a material that indicates the amount of heat required to raise the temperature of a unit mass of the substance by one degree Celsius. It is fundamental in calculations that relate heat exchange to temperature changes using the equation q = mc?T.

Heat Transfer and Energy Conservation

This concept involves the movement of thermal energy into or out of a system. In thermodynamics, when heat is added or removed, the energy conservation principle applies, stating that energy cannot be created or destroyed, only transferred, which results in a change in the system's temperature.

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