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33.9 kJ/mol at 25 °C 30.77 kJ/mol at 80.1 °C Std entropy change of vaporization, Δ vap S o: 113.6 J/(mol·K) at 25 °C 87.1 J/(mol·K) at 80.1 °C Solid properties Std enthalpy change of formation, Δ f H o solid? kJ/mol Standard molar entropy, S o solid: 45.56 J/(mol K) Heat capacity, c p: 118.4 J/(mol K) at 0 °C Liquid properties Std ...
However, a common temperature and pressure in use by NIST for thermodynamic experiments is 298.15 K (25 °C, 77 °F) and 1 bar (14.5038 psi, 100 kPa). [4] [5] NIST also uses 15 °C (288.15 K, 59 °F) for the temperature compensation of refined petroleum products, despite noting that these two values are not exactly consistent with each other.
This is a list of cities by average temperature (monthly and yearly). The temperatures listed are averages of the daily highs and lows. Thus, the actual daytime temperature in a given month may be considerably higher than the temperature listed here, depending on how large the difference between daily highs and lows is.
Anders Celsius's original thermometer used a reversed scale, with 100 as the freezing point and 0 as the boiling point of water.. In 1742, Swedish astronomer Anders Celsius (1701–1744) created a temperature scale that was the reverse of the scale now known as "Celsius": 0 represented the boiling point of water, while 100 represented the freezing point of water. [5]
According to British Standards, correctly calibrated, used and maintained liquid-in-glass thermometers can achieve a measurement uncertainty of ±0.01 °C in the range 0 to 100 °C, and a larger uncertainty outside this range: ±0.05 °C up to 200 or down to −40 °C, ±0.2 °C up to 450 or down to −80 °C.
To convert heat values to joules per mole values, multiply by 44.095 g/mol. To convert densities to moles per liter, multiply by 22.678 cm 3 mol/(L·g). Data obtained from CRC Handbook of Chemistry and Physics , 44th ed. pages 2560–2561, except for critical temperature line (31.1 °C) and temperatures −30 °C and below, which are taken from ...
Higashi anomalies: The very high c values that are labeled as thermal conductivities in table III on page 100 would roughly fit the thesis of the paper if they came with lower orders of magnitude. The way that the dry soils get a lot lighter between Table I on page 99 and table IV on pages 102-3 is eventually explained by the fact that Table I ...
Temperature-dependency of the heats of vaporization for water, methanol, benzene, and acetone. In thermodynamics, the enthalpy of vaporization (symbol ∆H vap), also known as the (latent) heat of vaporization or heat of evaporation, is the amount of energy that must be added to a liquid substance to transform a quantity of that substance into a gas.