Heat Capacity and Calorimetry - AP Chemistry

$C = \frac{q}{\triangle T}$. Heat capacity is the ratio of heat absorbed to temperature change.

Use $q_{\text{reaction}} = -C_{\text{cal}} \times \Delta T$. Uses total calorimeter heat capacity for precise energy measurement.

Heat absorbed or released. Standard symbol for heat energy in thermodynamic calculations.

Use calorimetry to find $c$ from $q = m \times c \times \Delta T$. Heat known metal in calorimeter and measure temperature change.

Joules per gram per degree Celsius (J/g°C). Standard SI units for energy per unit mass per temperature change.

To measure the heat of chemical reactions or physical changes. Primary purpose is precise measurement of thermal energy changes.

Energy cannot be created or destroyed; it is conserved. Fundamental principle stating total energy remains constant in isolated systems.

$q = m \times c \times \triangle T$. Fundamental equation for calculating thermal energy transfer.

$C = m \times c$. Heat capacity equals mass times specific heat capacity.

To measure the heat of combustion reactions. Specialized for high-energy combustion reactions requiring sealed conditions.

Sum of $q$ for temperature change and $q$ for phase change. Both sensible and latent heat contributions must be included.

To measure heat of reaction at constant volume. Bomb calorimeter operates under constant volume conditions.

Determining enthalpy changes of reactions. Essential application for studying reaction thermodynamics.

$C_{\text{cal}} = \frac{q}{\triangle T}$ for the calorimeter. Determined by measuring heat and temperature change for the calorimeter.

$\triangle H = q_{\text{p}}$. At constant pressure, heat equals enthalpy change.

Use $c = \frac{q}{m \times \triangle T}$. Rearrangement of the basic calorimetry equation.

Acts as the medium absorbing or releasing heat. Water's high heat capacity makes it ideal for absorbing reaction heat.

$q = m \times \triangle H_{\text{transition}}$. Where $\triangle H_{\text{transition}}$ is the specific enthalpy of phase change.

$q = m \times c \times \triangle T$. Where $q$ is heat, $m$ is mass, $c$ is specific heat, and $\triangle T$ is temperature change.

Heat lost by the system equals heat gained by the surroundings. Based on conservation of energy in thermal equilibrium.

$q_{\text{reaction}} = -(q_{\text{water}} + q_{\text{cal}})$. Accounts for heat absorbed by both water and calorimeter.

$\triangle U = q_{\text{v}}$. At constant volume, heat equals internal energy change.

Heat capacity is total heat required, specific is per gram. Heat capacity is extensive, specific heat is intensive property.

No heat is lost to the surroundings. Ideal calorimeter assumption for simplified calculations.

Heat capacity of the calorimeter. Standard notation for calorimeter's heat capacity.

Measure $\triangle T$ and calculate $q$ using solution mass and $c$. Dissolution process measured by temperature change of solution.

Bomb calorimeter operates at constant volume, coffee cup at constant pressure. Different conditions affect which thermodynamic quantity is measured.

Pressure remains constant throughout the experiment. Open system allows pressure equilibrium with atmosphere.

Indicates heat is released by the system. Negative sign indicates exothermic process with energy release.