Asolution of water (kf=1.86 ∘c/m) and glucose freezes at − 4.15 ∘c. what is the molal concentration of glucose in this solution? assume that the freezing point of pure water is 0.00 ∘c.

The formula for depression of freezing point is:

   -(1)

where, is depression of freezing point, is freezing point depression constant and is molality.

Freezing point of pure water =  (given)

Freezing point of glucose =  (given)

Depression of freezing point, =

Substituting the values:

Substituting the values in formula (1):

Hence, the the molal concentration of glucose in the given solution is .

the atomic number will stay the same no matter how many electrons it has, so it doesn’t decrease nor increase. it’ll only change with a different number of protons

consider the reaction below.

 no rx

at 500 k, the reaction is at equilibrium with the following concentrations.

[pci5]= 0.0095 m

[pci3] = 0.020

[ci2] = 0.020 m

what is the equilibrium constant for the given reaction?

0.042

0.42

2.4

24