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Calorimetry

Calorimetry

When objects at different temperatures are placed in contact with each other but isolated from everything else, they attain thermal equilibrium. A container that prevents heat transfer in or out is called a calorimeter, and the use of a calorimeter to make measurements is called calorimetry. Generally, these measurements involve heat or specific heat capacity. The term "calorimetry problem" is used for any problem where the specified objects are thermally isolated from their surroundings. An...

Constant Pressure Calorimetry

Constant Pressure Calorimetry

Calorimetry is a technique used to measure the amount of heat involved in a chemical or physical process or to measure the heat transferred to or from a substance. The heat is exchanged with a calibrated and insulated device called the calorimeter. Calorimetry experiments are based on the assumption that there is no heat exchange between the insulated calorimeter and the external environment. The well-insulated calorimeters prevent the transfer of heat between the calorimeter and its external...

States of Matter and Phase Changes

States of Matter and Phase Changes

The internal energy of a substance—the total kinetic energy of all its molecules and the potential energy of their associated forces—depends on the strength of the intermolecular forces in the condensed phases and the pressure exerted on the substance. The internal energy of a substance is the highest in the gaseous state, the lowest in the solid state, and intermediate in the liquid state. Phase transitions are caused by changes in physical conditions, such as temperature and pressure, that...

Phase Transitions: Melting and Freezing

Phase Transitions: Melting and Freezing

Heating a crystalline solid increases the average energy of its atoms, molecules, or ions, and the solid gets hotter. At some point, the added energy becomes large enough to partially overcome the forces holding the molecules or ions of the solid in their fixed positions, and the solid begins the process of transitioning to the liquid state or melting. At this point, the temperature of the solid stops rising, despite the continual input of heat, and it remains constant until all of the solid is...

Phase Transitions: Sublimation and Deposition

Phase Transitions: Sublimation and Deposition

Some solids can transition directly into the gaseous state, bypassing the liquid state, via a process known as sublimation. At room temperature and standard pressure, a piece of dry ice (solid CO2) sublimes, appearing to gradually disappear without ever forming any liquid. Snow and ice sublimate at temperatures below the melting point of water, a slow process that may be accelerated by winds and the reduced atmospheric pressures at high altitudes. When solid iodine is warmed, the solid sublimes...

Phase Changes

Phase Changes

Phase transitions play an important theoretical and practical role in the study of heat flow. In melting or fusion, a solid turns into a liquid; the opposite process is freezing. In evaporation, a liquid turns into a gas; the opposite process is condensation.
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Related Experiment Video

Updated: Jul 11, 2026

Phase Diagram Characterization Using Magnetic Beads as Liquid Carriers

Phase Diagram Characterization Using Magnetic Beads as Liquid Carriers

Published on: September 4, 2015

Calorimetric measurement of the energy difference between two solid surface phases.

Y Y Yeo, C E Wartnaby, D A King

Science (New York, N.Y.)

|June 23, 1995

Summary

Researchers measured the energy difference between two platinum surface structures using a new calorimeter. The stable Pt{100}-hex phase is more stable than the Pt{100}-(1x1) phase by 20-25 kJ/mol.

Area of Science:

Surface science
Physical chemistry
Materials science

Background:

The Pt{100} surface exhibits different structural phases.
Understanding the energy differences between these phases is crucial for catalysis and surface chemistry.

Purpose of the Study:

To quantify the energy difference between the reconstructed Pt{100}-hex phase and the metastable Pt{100}-(1x1) phase.
To utilize a newly developed single-crystal surface calorimeter for precise surface energy measurements.

Main Methods:

Employed a single-crystal surface calorimeter to measure heats of adsorption.
Adsorbed carbon monoxide (CO) and ethylene (C2H4) on both Pt{100}-hex and Pt{100}-(1x1) surfaces.
Calculated surface energy differences based on differential heats of adsorption.

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Thermal Scanning Conductometry (TSC) as a General Method for Studying and Controlling the Phase Behavior of Conductive Physical Gels

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Main Results:

The energy difference between the clean Pt{100}-hex and Pt{100}-(1x1) surfaces was determined.
The Pt{100}-hex phase was found to be more stable than the Pt{100}-(1x1) phase.
Measured energy differences of 20 +/- 3 kJ/mol (for CO) and 25 +/- 3 kJ/mol (for C2H4) per surface platinum atom.

Conclusions:

The study successfully quantified the surface energy difference between two distinct Pt{100} phases.
The results provide valuable thermodynamic data for understanding platinum surface reconstructions.
The findings have implications for heterogeneous catalysis where surface structure influences reactivity.