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With $A={\lambda }_{33}$, $B={\lambda }_{34}{n}_4$ and $C={\lambda }_{11}{n}_1^2/2$, helium-3 evolves as ${\dot{n}}_3=C-A{n}_3^2-B{n}_3$ after deuterium elimination. The positive root is its unique attracting equilibrium for a fixed background. In the pp-I limit it reduces to $n_1\sqrt{{\lambda }_{11}/(2{\lambda }_{33})}$, making equilibrium abundance strongly temperature dependent.

A small abundance displacement from the helium-3 equilibrium abundance obeys $\dot{x}=-x/\tau$ to linear order. Rapid relaxation relative to background evolution allows the abundance to track its equilibrium. If the equilibrium drifts, the displacement equation also contains $-{\dot{n}}_{3e}$. In the pp-I limit the rate is $n_1\sqrt{2{\lambda }_{11}{\lambda }_{33}}$, so both production and destruction temperature dependences matter.

David Morris Lee, Douglas Dean Osheroff and Robert Coleman Richardson compressed coexisting liquid and solid helium-3 in a cell precooled by a dilution refrigerator. Helium-4 pressure drove coupled bellows and a piston; a capacitance diaphragm gauge read pressure and platinum nuclear magnetic resonance supplied thermometry. Uniform compression revealed a slope break A and a small pressure drop B; decompression and varied solid fraction checked reproducibility. Their April 1972 paper, Evidence for a New Phase of Solid He3, interpreted a new solid phase, without establishing liquid superfluidity. ^[ref]

The October follow-up replaced the thermometer assembly with a sample nuclear magnetic resonance coil. An applied magnetic field gradient selected different sample layers, separating strong solid signals from the liquid background. At A the liquid resonance shifted; at B its shift disappeared and its magnetic susceptibility fell. Removing the gradient resolved the frequency shift directly. Independence from solid fraction and distinct relaxation times supported the liquid assignment. Thus the reinterpretation rested on phase-selective evidence, rather than relabeling the first paper's title. These magnetic observations identify changed liquid phases; they do not directly measure frictionless flow. ^[ref]

Douglas Dean Osheroff recalls the subsequent p-wave interpretation. ^[ref]

The inference has a useful limit. A pressure anomaly in two coexisting phases cannot, by itself, identify which phase changed: both contribute to the common phase coexistence curve. Thermometer lag, a temperature gradient or slow equilibration can also separate indicated temperature from the sample state. Correlating another response with the anomaly provides information that repeating the same pressure trace cannot supply. Conversely, a shifted magnetic resonance alone does not measure a frictionless flow rate.

Loss of mechanical integrity associated with retained helium, including the growth and coalescence of gas-containing cavities at grain boundaries. Gas location, trapping, temperature, stress and the initial microstructure influence the result. It can occur in austenitic steel without the ferritic ductile-to-brittle transition.^[ref]

Helium liquefaction converts helium gas into a collectable liquid. It creates a bath for investigating material properties at very low temperatures, including superconductivity. The central question is how the incoming specific enthalpy compares with the specific enthalpies of the outgoing liquid and vapor. The liquefaction enthalpy budget makes that comparison explicit; a temperature decrease by itself does not specify a liquid yield.

In a Joule-Thomson effect cooling stage, a throttling pressure drop approximately preserves enthalpy under the assumptions of the steady-flow energy balance. For an ideal gas, specific enthalpy depends only on temperature: with positive specific heat capacity at constant pressure, equal specific enthalpy means equal temperature. Thus its Joule-Thomson coefficient is zero. An ideal gas also supplies no liquid branch. Cooling by throttling depends on real gas properties; expansion is not an automatic source of refrigeration.

For a local drop $dp<0$, $dT={\mu }_{\mathrm{JT}}dp$ cools only where the Joule-Thomson coefficient is positive. Precooling must bring the real gas into a useful cooling region, with enough cooling to overcome unwanted heat transfer. A finite expansion can cross a Joule-Thomson inversion curve; its final state requires the full enthalpy balance, including phase coexistence if liquid forms. Kamerlingh Onnes's 1908 helium liquefaction experiment combined external precooling with regeneration to reach that regime. The Joule-Thomson effect article develops the throttling identities and their assumptions.

During radiation domination, the weak conversion rate scales as $T^5$ whereas the Hubble parameter scales as $\sqrt{G{g}_{\ast }}{T}^2$. Their crossing fixes the cosmological weak freeze-out temperature. A faster expansion raises it, leaving a larger neutron-to-proton ratio, and shortens the interval for free-neutron decay after freeze-out. Both effects increase the helium-4 mass fraction if the extra component does not independently change reaction rates or inject decay products.

Pyotr Leonidovich Kapitza's 1938 test compared helium flow through optically flat glass disks. Suspension set the tube-to-bath level difference; a cathetometer read levels. The gap was estimated as $0.5\mu \mathrm{m}$. Levels barely moved over minutes above the transition, but equalized in seconds below. A laminar flow viscosity calculation gave only an upper bound.^[ref]

The essential control is to compare the same restriction and level readout at different temperatures. A changed pressure head is not itself evidence for a changed material response: the driving head must be included when interpreting the flow. For an idealized comparison at equal vapor pressure, negligible surface tension corrections and nearly constant mass density $\rho$, hydrostatic equilibrium givesHere $\Delta h$ is the difference in free-surface heights and $g$ is gravitational acceleration. This explains why following a liquid level provides both a driving pressure and a transported volume; it does not turn a finite-resolution observation into proof of zero viscosity.

The Helmholtz free energy iswhere $U$ is internal energy, also denoted $E$ elsewhere here, $T$ is absolute temperature, and $S$ is entropy. For the closed system of fixed composition and only pressure-volume work described above, spontaneous relaxation at fixed temperature and volume cannot increase $F$. Stable thermodynamic equilibrium is a global minimum over the permitted alternatives, including different thermodynamic phases. A rigid vessel fixes the total volume; it does not require each coexisting thermodynamic phase to retain its own volume.

For a constructed comparison at $300\mathrm{K}$, suppose one candidate has $1.5\mathrm{kJ}$ more internal energy but $6\mathrm{J}{\mathrm{K}}^{-1}$ more entropy than another at the same temperature and volume. Its difference isThus the candidate with higher internal energy has lower Helmholtz free energy. This is the practical reason for retaining the entropy term when selecting a state.

For equilibrium states within a smooth branch of fixed composition, the first law of thermodynamics gives $dU=TdS-pdV$, henceThese derivatives extract entropy and pressure; the differential is not an evolution equation for relaxation. If chemical species amounts $n_i$ vary, add ${\sum }_i{\mu }_{i}d{n}_i$, with molar chemical potentials ${\mu }_i$. A closed system can still change chemical species amounts through chemical reactions; the fixed-composition simplification then needs the conserved-inventory constraints of chemical equilibrium. See MIT 5.60, Lecture 14, fundamental equations and chemical potentials.

The minimum principle has a short explanation. At fixed volume, no boundary work occurs, so $Q=\Delta U$. A thermal reservoir at positive temperature $T$ loses entropy $Q/T$. Consequentlyby the Second law of thermodynamics. Here both endpoint states share the imposed temperature. See MIT 5.60, Lecture 12, criteria for spontaneous change.

The microscopic counterpart is $F=-k_{B}T\ln Z$ in the canonical ensemble, with Boltzmann constant $k_B$ and partition function $Z$. The partition function examples compute the balance between internal energy and entropy; the chemical equilibrium example already displays an ideal-mixture Helmholtz free energy minimum.

The Henderson-Hasselbalch equation estimates buffer solution pH using a weak acid's acid dissociation constant and the conjugate base to weak acid concentration ratio.

Its activity form is an exact rearrangement of the chosen chemical equilibrium relation. Write the acid dissociation step as $\mathrm{HA}\rightleftharpoons {\mathrm{H}}^{+}+{\mathrm{A}}^{-}$, with hydrated hydrogen ions understood in water and the solvent convention incorporated into the acid dissociation constant. For consistent standard states,Here each $a_i$ is a dimensionless thermodynamic activity at chemical equilibrium. Exactness refers to this specified acid dissociation constant relation and the chosen single-ion thermodynamic activity convention, not to identifying the ratio with quantities initially mixed. If water is instead written explicitly as a reactant, its thermodynamic activity must be treated consistently. See Hippler and Metcalfe, Using activities to correct the Henderson-Hasselbalch equation (2020), equations 3–4.

For a toy weak acid with stipulated pKa $5$, use the ideal dilute concentration approximation and put $r=[{\mathrm{A}}^{-}]/[\mathrm{HA}]$. The Henderson-Hasselbalch equation becomes $\mathrm{pH}\approx 5+{\log }_{10}r$:More conjugate base relative to weak acid means higher pH. Each tenfold increase in the ratio contributes exactly one to the calculated pH. The stipulated pKa is not a tabulated value for an identified substance.

The distinction between thermodynamic activity and concentration is explicit when $a_i={\gamma }_i[i]/c^{\circ }$, where ${\gamma }_i$ is an activity coefficient and $c^{\circ }$ is the reference concentration:Neglecting the final term gives the usual approximate Henderson-Hasselbalch equation. It is justified when the ratio of activity coefficients is sufficiently close to one, as in a suitable dilute ideal approximation. Ionic strength, including contributions from other dissolved ions, affects activity coefficients; a nominally dilute weak acid alone does not establish that all corrections are small. The ratio must use chemical equilibrium concentrations. Replacing these by prepared amounts or post-neutralization inventories is a further approximation, suitable only when subsequent redistribution is small. See Hippler and Metcalfe, concentration, activity, and analytical-concentration approximations.

The short derivation is to solve the acid dissociation constant relation for $a_{{\mathrm{H}}^{+}}$, take a negative base-ten logarithm, and use the definitions of pH and pKa. Its useful beauty is that a chemical equilibrium becomes a simple rule about a ratio: select a weak acid with pKa near the desired pH, then adjust the partner ratio. Scaling both partner concentrations equally leaves the ideal pH prediction unchanged, while changing buffer capacity. In practical buffer solutions, temperature, ionic strength, and the available inventories still matter.

A Hertzsprung-Russell diagram plots stellar luminosity against effective temperature or spectral type. By convention, temperature usually decreases from left to right.

For a stellar homology sequence with $R\propto M^X$ and $L\propto M^Y$, the Stefan–Boltzmann law gives $T_{\mathrm{eff}}\propto M^{(Y-2X)/4}$. Eliminating mass gives the displayed Hertzsprung-Russell diagram slope when $Y\ne 2X$. The usual horizontal axis decreases in temperature toward the right, reversing the visual left-to-right sign. The relation is between logarithmic variables and depends on the specified structural assumptions.

Victor Franz Hess's 1912 series used two sealed, 3-mm-walled ionization chambers with Theodor Wulf's fiber electrometers. Karl Bergwitz suggested internal plating; Günther & Tegetmeyer improved focusing. Basket-mounted ground comparisons, insulation-loss measurements, simultaneous detectors and barograph-derived heights supplied checks. The highest flight reached 5350 m; its comparisons came from Vienna and after landing, without a launch-site baseline.^[ref]

A third, thin-walled chamber admitted ambient air. Hess multiplied its readings by $750/b$, with pressure $b$ in millimeters of mercury, warning that vessel-wall contributions might violate this scaling. He recorded outside temperature but applied no absolute-temperature correction. Night flights, an eclipse and weather observations constrained alternatives to radiation from above; the eclipse argument addressed directly propagating solar radiation.^[ref]

The electrometers read gradual electric potential loss caused by continuing air ionization. The low-altitude dip and strong high-altitude rise favored an extraterrestrial contribution, without measuring proton composition.^[ref] An ionization chamber integrates electric charge: one energetic particle may create many ion pairs, several particles may contribute to one reading, and a photon can create charged particles in the gas or walls. A voltage-loss reading is therefore neither a count of primary cosmic rays nor a chemical analysis of them.

Domenico Pacini supplied independent evidence: in June 1911 he compared a copper-box-enclosed electroscope at the sea surface and 3 m underwater, more than 300 m offshore above an 8-m-deep seabed. Reduced underwater ionization, stable electrical loss between runs, and a lake comparison supported an external contribution independent of soil radioactive decay. Water provided shielding; this established a different constraint from Hess's altitude comparison.^[ref]

Hess's law states that compatible chemical reaction enthalpies add when their equations add. Reversing a chemical reaction reverses its enthalpy change; multiplying the entire chemical reaction equation by a factor multiplies that change by the same factor. The reason is that enthalpy is a state function: intermediate states cancel from the differences. A cycle supplies one independent balance relation; it cannot determine two unknown inputs without further information.

The law is named after Germain Henri Hess.

For specified initial and final thermodynamic states, the change is $\Delta H=H_{\mathrm{final}}-H_{\mathrm{initial}}$. Because enthalpy is an extensive variable, a quoted reaction $\Delta H$ belongs to the amount of substance specified for each species in its chemical equation. Reversing the equation changes the sign; scaling every coefficient scales $\Delta H$; adding compatible equations adds their $\Delta H$ values. A per-mole value must say which chemical equation and normalization it uses. Match temperature, pressure, thermodynamic phases, chemical solution compositions and reference states before cancellation; the same formula in a gas and a liquid represents different states.^[ref]

The value of Hess's law is that an inaccessible reaction enthalpy can be obtained from measurable transformations. The algebra does not require those transformations to be steps of the actual reaction mechanism. Neither an activation energy nor a reaction rate follows from the endpoint difference: a catalyst may change the reaction rate while preserving the compatible initial and final enthalpies.

A practical test compares three transformations involving sodium hydroxide: dissolution of the solid, neutralization of its chemical solution by hydrochloric acid, and reaction of the solid directly with hydrochloric acid. In the ideal compatible-state notation, the hydrogen ion and hydroxide giveThe hydroxide cancels, whereas the newly formed water remains. Sodium and chloride spectator ions must still be included in the full material inventory when matching actual chemical solutions.

The teaching protocol Calorimetry: Heat of Neutralization Reaction & Hess's Law, Procedure A–C, uses nested insulated cups, a cardboard lid and a thermometer. It mixes $75\mathrm{mL}$ each of $2.0\mathrm{mol}{\mathrm{L}}^{-1}$ hydrochloric acid and sodium hydroxide chemical solutions; separately it adds $6.00\mathrm{g}$ solid sodium hydroxide to diluted hydrochloric acid, or to $150\mathrm{mL}$ water. It records initial temperatures, stirs, reads temperature every $30\mathrm{s}$, repeats runs, and extrapolates cooling trends to mixing time. Rapid weighing limits moisture uptake. The Introduction neglects vessel heat capacity and room losses; these are approximations, not a measured calibration. The readout tests whether the inferred enthalpies add, rather than directly measuring a state function.^[ref]

Matching the chemical equations alone is insufficient. The direct-acid recipe uses $0.160\mathrm{mol}$ hydrochloric acid, whereas the solution-mixing recipe uses $0.150\mathrm{mol}$. The dissolution run also does not automatically reproduce the water inventory of the mixed-solution run. Exact closure requires matching initial and final chemical solution compositions and adding any necessary mixing or dilution enthalpies. Agreement after approximate corrections is a limited test, rather than proof of exact cancellation for those recipes.

To improve the calorimetry, use calorimeter calibration for the participating hardware, and estimate calorimeter heat-loss correction under comparable conditions. With an approximately constant total receiving heat capacity $C_{\mathrm{tot}}=m{c}_p+C_{\mathrm{cal}}$, common initial temperature, constant external pressure, only expansion work, negligible escaping material and negligible bulk kinetic energy and potential energy changes, the balance isHere $m$ is the chemical solution mass, $c_p$ its specific heat capacity at constant pressure, $C_{\mathrm{cal}}$ the hardware heat capacity, and $Q_{\mathrm{loss},\mathrm{out}}$ the signed outward heat loss. Different initial temperatures require separate warming terms. Calorimeter calibration and matching chemical solution compositions address different errors.

For an original constructed model, choose $C_{\mathrm{tot}}=120\mathrm{J}{\mathrm{K}}^{-1}$ and $\Delta T=3\mathrm{K}$. Neglect outward heat loss and other corrections. The receiving chemical solution and hardware gain $q_{\mathrm{receiver}}=360\mathrm{J}$, so $q_{\mathrm{rxn}}=-360\mathrm{J}$. If the completed extent of reaction is $\xi =0.020\mathrm{mol}$ for a unit-coefficient chemical equation, the inferred reaction enthalpy per mole of that reaction isThese chosen numbers illustrate the signs and normalization; they are not measured sodium hydroxide data and are independent of the abstract $A,B,C$ example.

A loss of heat to the room makes the uncorrected warming underestimate the magnitude of a heat-releasing reaction. Incomplete dissolution, incomplete reaction, uncertain amount of substance, or a slow thermometer response can also spoil closure. A useful experimental residual is $r=\Delta H_{\mathrm{direct}}-(\Delta H_D+\Delta H_N)$ after all changes have been placed on the same amount and state basis. Compare $r$ with the measurement uncertainty, accounting for shared calibration errors; averaging repeated runs reduces scatter without removing a common bias.

Variation of body temperature across times or body regions. An endothermic animal need not maintain one constant temperature continuously.

Ordinary atmospheric snow crystals are predominantly hexagonal ice Ih. Rotating by sixty degrees around its crystallographic axis leaves the equilibrium orientation dependence unchanged, giving six equivalent basal-plane directions. Temperature and supersaturation determine whether plates, columns or crystal dendrites develop. Dendritic growth of a snowflake needs this crystal symmetry as well as the diffusion instability.

When collisions thermalize an optically thin two-level atom, the upper fraction is $f_u=g{e}^{-\theta /T}/(1+g{e}^{-\theta /T})$ and the emitted power per atom is $A_{21}\Delta E{f}_u$. Its logarithmic temperature slope is $(\theta /T)(1-f_u)>0$. Radiative cooling still occurs, but collision frequency no longer sets the emitted power as in the low-density limit.

High-pressure experimental metrology connects three tasks: producing pressure, retaining it without leakage, and assigning a calibrated value to the pressure experienced by a sample. A large applied force alone establishes none of the last two. The useful result is a reproducible material property at specified pressure, temperature and stress conditions, with stated measurement uncertainty.

Percy Williams Bridgman identified leakage as an earlier experimental limit. His 1946 lecture describes packing that tightens as pressure rises, ultimately leaving vessel strength as a limit.^[ref]

The Bridgman unsupported-area seal turns the very pressure that would drive a leak into an extra seating force. Its appeal is a feedback between load and sealing, rather than an assumption of perfectly fitted rigid surfaces. The piston-cylinder pressure apparatus below explains that feedback; pressure calibration then separates the applied load from the sample's inferred pressure.

High-temperature superconductivity is a historical name for superconductivity above earlier metallic benchmarks. The original Bednorz-Müller experiment operated at tens of kelvins, requiring deep cooling; cuprate superconductors opened a new materials family.^[ref]

A higher superconducting transition temperature enlarges the available operating range, but useful transport also needs a sufficient superconducting critical current at the operating temperature and magnetic field. In a ceramic, connections between grains can limit the whole specimen even when individual grains support superconductivity. This connects the materials problem to superconducting weak links and the Josephson effect. The parallel-path model of a superconducting ceramic below isolates why connectivity matters.