Thermochemistry and Calorimetry

This set of flashcards focuses on key concepts and vocabulary related to thermochemistry and calorimetry, including specific heat, the heat equation, and heat transfer.

Calorimetry

The experimental measurement of the heat of chemical reactions or physical changes.

Heat equation

Q = m c Δt, where Q is heat, m is mass, c is specific heat capacity, and Δt is the change in temperature.

Δt (Delta t)

The change in temperature, calculated as final temperature minus initial temperature.

Specific heat capacity (c)

The amount of heat needed to raise the temperature of one gram of a substance by one degree Celsius.

Positive Q value

Indicates that heat is gained by the substance, leading to an increase in temperature.

Negative Q value

Indicates that heat is lost by the substance, leading to a decrease in temperature.

Specific heat of Aluminum

0.903 joules per gram per degree Celsius, indicating its heat absorption capability.

Insulator

A material with high specific heat, preventing rapid temperature changes.

Conductor

A material with low specific heat, allowing heat to transfer quickly.

Heat loss calculation

Using the formula Q = m c Δt to determine the heat exchanged by the substance.

Room temperature

Typically around 25 degrees Celsius, often used as a reference point in calorimetry experiments.