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This is due to hydrogen bonding dominating the intermolecular forces, which results in a packing of molecules less compact in the solid. The density of ice increases slightly with decreasing temperature and has a value of 0.9340 g/cm 3 at −180 °C (93 K). [7] When water freezes, it increases in volume (about 9% for fresh water). [8]
The density of ice I h increases when cooled, down to about −211 °C (62 K; −348 °F); below that temperature, the ice expands again (negative thermal expansion). [ 5 ] [ 6 ] Besides ice I h , a small amount of ice I c may occasionally present in the upper atmosphere clouds. [ 140 ]
The density of dry ice increases with decreasing temperature and ranges between about 1.55 and 1.7 g/cm 3 (97 and 106 lb/cu ft) below 195 K (−78 °C; −109 °F). [3] The low temperature and direct sublimation to a gas makes dry ice an effective coolant, since it is colder than water ice and leaves no residue as it changes state. [4]
Both brine and air volumes influence sea-ice density values, which are typically around 840–910 kg/m 3 for first-year ice. Sea-ice density is a significant source of errors in sea-ice thickness retrieval using radar and laser satellite altimetry, resulting in uncertainties of 0.3–0.4 m. [21]
Under increasing pressure, ice undergoes a number of transitions to other polymorphs with higher density than liquid water, such as ice II, ice III, high-density amorphous ice (HDA), and very-high-density amorphous ice (VHDA). [38] [39] Temperature distribution in a lake in summer and winter
Ice: 916.7: At temperature < 0 °C Cooking oil: 910–930: Sodium: 970: Water (fresh) 1,000: At 4 °C, the temperature of its maximum density ... Air density vs ...
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Specific heat capacity often varies with temperature, and is different for each state of matter. Liquid water has one of the highest specific heat capacities among common substances, about 4184 J⋅kg −1 ⋅K −1 at 20 °C; but that of ice, just below 0 °C, is only 2093 J⋅kg −1 ⋅K −1.