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Related Concept Videos

Hydrogen Bonds01:04

Hydrogen Bonds

A hydrogen bond is formed when a weakly positive hydrogen atom already bonded to one electronegative atom (for example, the oxygen in the water molecule) is attracted to another electronegative atom from another polar molecule, such as water (H2O), hydrogen fluoride (HF), or ammonia (NH3). The huge electronegativity difference between the H atom (2.1) and the atom to which it is bonded (4.0 for an F atom, 3.5 for an O atom, or 3.0 for an N atom), combined with the very small size of an H atom...
Hydrogen Bonds00:26

Hydrogen Bonds

Hydrogen BondsHydrogen bonds are weak attractions between atoms that have formed other chemical bonds. One of these atoms is electronegative, like oxygen, and has a partial negative charge. The other is a hydrogen atom that has bonded with another electronegative atom and has a partial positive charge.Hydrogen Bonds Control the World!Because hydrogen has very weak electronegativity when it binds with a strongly electronegative atom, such as oxygen or nitrogen, electrons in the bond are...
Intermolecular Forces03:13

Intermolecular Forces

Atoms and molecules interact through bonds (or forces): intramolecular and intermolecular. The forces are electrostatic as they arise from interactions (attractive or repulsive) between charged species (permanent, partial, or temporary charges) and exist with varying strengths between ions, polar, nonpolar, and neutral molecules. The different types of intermolecular forces are ion–dipole, dipole–dipole, hydrogen bonds, and dispersion; among these, dipole–dipole, hydrogen bonds, and dispersion...
Comparing Intermolecular Forces: Melting Point, Boiling Point, and Miscibility02:34

Comparing Intermolecular Forces: Melting Point, Boiling Point, and Miscibility

Intermolecular forces are attractive forces that exist between molecules. They dictate several bulk properties, such as melting points, boiling points, and solubilities (miscibilities) of substances. Molar mass, molecular shape, and polarity affect the strength of different intermolecular forces, which influence the magnitude of physical properties across a family of molecules.
Temporary attractive forces like dispersion are present in all molecules, whether they are polar or nonpolar. They...
Hybridization of Atomic Orbitals I03:24

Hybridization of Atomic Orbitals I

The mathematical expression known as the wave function, ψ, contains information about each orbital and the wavelike properties of electrons in an isolated atom. When atoms are bound together in a molecule, the wave functions combine to produce new mathematical descriptions that have different shapes. This process of combining the wave functions for atomic orbitals is called hybridization and is mathematically accomplished by the linear combination of atomic orbitals. The new orbitals that...
Predicting Molecular Geometry02:27

Predicting Molecular Geometry

VSEPR Theory for Determination of Electron Pair Geometries

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A Microfluidic Approach for the Study of Ice and Clathrate Hydrate Crystallization
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Molecular hydrogen storage in binary THF-H2 clathrate hydrates.

Timothy A Strobel1, Craig J Taylor, Keith C Hester

  • 1Center for Hydrate Research, Colorado School of Mines, Golden, Colorado 80401, USA.

The Journal of Physical Chemistry. B
|August 25, 2006
PubMed
Summary

Binary tetrahydrofuran (THF)-hydrogen clathrate hydrates store up to 1.0 wt % hydrogen. THF molecules preferentially occupy large cavities, limiting further hydrogen storage in small cavities.

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Area of Science:

  • Materials Science
  • Chemical Engineering
  • Physical Chemistry

Background:

  • Clathrate hydrates offer potential for hydrogen storage.
  • Binary hydrates, such as THF-H(2), are investigated for enhanced storage capacity.
  • Understanding guest molecule interactions within hydrate cages is crucial.

Purpose of the Study:

  • To determine the hydrogen storage capacity of binary THF-H(2) clathrate hydrate.
  • To investigate the influence of formation pressure, THF composition, and time on hydrogen storage.
  • To elucidate the preferential occupation of hydrate cages by THF and H(2).

Main Methods:

  • Experimental determination of hydrogen storage capacity.
  • Varying formation pressure, THF concentration, and experimental time.
  • Analysis of hydrogen uptake and hydrate structure.

Main Results:

  • Hydrogen storage capacity increases with pressure, reaching a plateau of approximately 1.0 wt % H(2).
  • This capacity corresponds to full occupancy of small 5(12) cages by H(2) and large 5(12)6(4) cages by THF.
  • Decreasing THF concentration did not enhance hydrogen storage, indicating THF's preference for large cages.

Conclusions:

  • THF-H(2) clathrate hydrate can store up to 1.0 wt % hydrogen at moderate pressures (<60 MPa).
  • THF molecules preferentially occupy the large hydrate cages, limiting further hydrogen incorporation.
  • The storage capacity is largely independent of initial THF concentration under tested conditions.