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11. Calorimetry

The chapter delves into the concepts of calorimetry, heat, and temperature, emphasizing the laws governing heat transfer and specific heat capacity. It covers the instruments used to measure heat exchanges, such as calorimeters, and discusses phase changes along with the associated latent heats. Additionally, the effects of pressure and impurities on states of matter are explored, along with the practical representation of temperature changes through cooling curves.

Sections

Calorimetry

Calorimetry deals with heat transfer and its measurement in physical and chemical changes.

11 Section Overview

Start current section content and materials

11.1 Heat and Temperature

Heat is the energy transferred between bodies due to temperature differences, while temperature measures the thermal condition of an object.

11.2 Principle of Calorimetry

Calorimetry relies on the principle that heat lost by a hot body equals the heat gained by a cold body, adhering to the conservation of energy.

11.3 Specific Heat Capacity (c)

Specific heat capacity measures the heat required to change the temperature of a substance.

11.4 Calorimeter

A calorimeter is a device used to measure heat exchange during physical and chemical changes.

11.5 Change of State

This section discusses how substances change from one physical state to another, highlighting the concepts of latent heat during processes like melting and boiling.

11.5.1 Melting (Fusion)

This section explains the process of melting (or fusion) where a solid turns into a liquid, emphasizing the concept of latent heat of fusion.

11.5.2 Boiling (Vaporization)

This section discusses boiling as a form of vaporization, detailing the heat required for a liquid to change into gas at its boiling point.

11.6 Latent Heat

Latent heat refers to the heat energy required for a substance to change its state without a change in temperature.

11.7 Effects of Pressure and Impurities on Change of State

This section discusses how pressure and impurities affect the melting and boiling points of substances.

11.8 Cooling Curve

A cooling curve graphically represents the change in temperature over time as a substance cools, illustrating plateaus during phase changes and sloped lines during temperature changes.

Learning Objectives

  • Heat is energy transferred due to a temperature difference.

  • The principle of calorimetry states that heat lost by a hot body equals the heat gained by a cold body.

  • Specific heat capacity quantifies the heat needed to raise the temperature of a substance.

Key Concepts

Heat

A form of energy transferred between bodies due to temperature differences.

Temperature

A measure of the thermal condition of a body, indicating how hot or cold it is.

Specific Heat Capacity

The amount of heat required to raise the temperature of 1 kg of a substance by 1°C or 1 K.

Latent Heat

The heat supplied or extracted during a phase change without temperature change.

Calorimeter

A device used for measuring the amount of heat exchanged in physical and chemical processes.

Practice Exercises

Total Questions

3

Estimated Time

6 min

Passing Score

70%

Instructions

  • Read each question carefully
  • You can use hints if you need help
  • Complete all questions before submitting