Electron Volt to Calorie (th)

Because subatomic energies in joules have absurdly small exponents — a visible-light photon carries about 3 × 10⁻¹⁹ J, but a convenient 1.9 eV. The electron volt is scaled to the quantum world, making numbers human-readable. It also doubles as a mass unit (via E = mc²): a proton is 938.3 MeV/c², far easier to work with than 1.673 × 10⁻²⁷ kg.

Visible light photons range from about 1.65 eV (deep red, 750 nm) to 3.1 eV (violet, 400 nm). Green light, where the human eye is most sensitive, sits around 2.3 eV. Ultraviolet photons start at 3.1 eV and can exceed 100 eV in the extreme UV. These energies are why UV can damage DNA (breaking molecular bonds of 3–5 eV) while visible light cannot.

A semiconductor's bandgap — the minimum energy to free an electron from its bond — is expressed in eV. Silicon has a bandgap of 1.12 eV, gallium arsenide 1.42 eV, and gallium nitride 3.4 eV. The bandgap determines which wavelengths of light a solar cell can absorb and what color an LED emits. Lower bandgap means longer-wavelength (redder) light.

The LHC accelerates protons to 6.5 TeV (6.5 × 10¹² eV) per beam, giving collisions a center-of-mass energy of 13 TeV. That sounds enormous, but 13 TeV is only about 2 microjoules — the kinetic energy of a flying mosquito. The power of the LHC lies in concentrating that energy into a space a million times smaller than an atom.

Multiply by 1.602 176 634 × 10⁻¹⁹. So 1 eV = 1.602 × 10⁻¹⁹ J, 1 keV = 1.602 × 10⁻¹⁶ J, and 1 MeV = 1.602 × 10⁻¹³ J. This conversion factor is exactly the elementary charge in coulombs, because an electron volt is defined as the energy gained by one electron charge crossing one volt of potential.

The thermochemical calorie (cal th) is defined as exactly 4.184 joules; the International Table calorie (cal IT) is exactly 4.1868 joules — a difference of 0.066%. The thermochemical value was fixed by the US National Bureau of Standards in 1935 for chemistry; the IT value was adopted for steam tables. In nutritional contexts, the difference is irrelevant, but in precise calorimetry it can matter.

Decades of published thermochemical data — heats of formation, bond energies, combustion enthalpies — are recorded in cal th and kcal th. Converting every reference table to joules would be error-prone and disruptive. Biochemistry textbooks still quote ATP hydrolysis at ~7.3 kcal/mol and glucose oxidation at ~686 kcal/mol. The convention persists because the existing literature is too vast to rewrite.

A dried, weighed food sample is sealed in a steel vessel filled with pure oxygen, submerged in a known mass of water. An electric spark ignites the sample, which burns completely. The temperature rise of the surrounding water — measured to 0.001°C — gives the total heat released. One degree rise per gram of water equals one calorie. Corrections for the heat capacity of the bomb itself, the ignition wire, and acid formation give results accurate to ±0.1%. Atwater then applied digestibility factors to convert bomb values to usable food energy.

Hydrogen releases about 34,000 cal th per gram; methane about 13,300 cal th/g; ethanol about 7,100 cal th/g; and glucose about 3,720 cal th/g. These values appear throughout chemistry textbooks as standard reference data. The higher the cal/g value, the more energy-dense the fuel — which is why hydrogen is attractive despite being hard to store.

Before 1935, the calorie was defined by water's heat capacity, which varies with temperature — the 15°C calorie, 20°C calorie, and mean calorie all differed slightly. The US National Bureau of Standards ended the ambiguity by defining the thermochemical calorie as exactly 4.184 J, a round value close to all the experimental variants. This gave chemists a fixed, reproducible conversion factor independent of water's quirky temperature-dependent heat capacity.