The temperature is 146 oC.
0.10m NaCl has a lower freezing temperature compared to 0.10m glucose. This is because NaCl dissociates into more particles in solution, causing greater osmotic pressure that lowers the freezing point more than glucose, which does not dissociate.
Melting (freezing) point: α-D-glucose: 146 °C β-D-glucose: 150 °C Glucose will decompose already below its boiling point, so there's no valued boiling point (at least not at normal pressure).
I suppose that barium chloride cause the greatest drop of the freezing point.
This quantity is equivalent to 90 g glucose / kg water = 0.50 mole particles of solute / kg water, so with a 'molar cryoscopic constant' for water of -1.86 oC/kgthis lowers the freezing point to -0.93 oC.
A solution of ethylene glycol would have the highest freezing point among the three options.
Freezing point.
The solution with glucose (C6H12O6) would have the lowest freezing point. This is because the number of particles in the solution contributes to the lowering of the freezing point, and glucose, being a covalent compound, dissociates into more particles in solution compared to the other compounds given.
what is the freezing point of lithuim?
The freezing point is the same as the melting point.
what is the freezing point of N2O
The freezing point is -252 degrees..................
what is irons freezing point