The temperature is 146 oC.
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.
50.5g of glucose glucose is 180.18 g/mol 50.5/180.18 = 0.280 mol glucose 0.280 mol glucose/0.475 kg H2O = 0.589 m which is molality deltaTsubF = (-1.86 degress C/m)(0.589) = -1.10 degrees C -1.10 degrees C + 0.00 degrees C = -1.10 degrees C as your freezing point seeing that 0.00 degrees is the standard freezing point of water deltaTsubB = (0.512 degrees C/m)(0.589) = 0.301568 it asks for 6 sig figs so 0.301568 degrees C + 100.000 degrees C (boiling point H2O) = 100.302 degrees C Mastering Chemistry sucks sometimes....
Glucose
what is the freezing point of N2O
the freezing point is 100
what is the freezing point of lithuim?
it is increased with the increasing density
The freezing point is the same as the melting point.
Freezing point is a synonym.
0oC is freezing point