A metal, , of atomic weight 96 reacts with fluorine to form a salt that can be represented as . In order to determine and therefore the formula of the salt, a boiling point elevation experiment is performed. A 9.18- sample of the salt is dissolved in 100.0 of water and the boiling point of the solution is found to be 374.38 . Find the formula of the salt.
You need to rework your post. No formula representation for the salt. No unit on 9.18 WHAT sample. No units on 374.38? . ETC.
To find the formula of the salt, we need to determine the value of the variable "n" in the formula M(n)F(6), where M represents the metal.
First, we need to calculate the change in boiling point (∆Tb) caused by the presence of the salt in the solution. This can be done using the formula:
∆Tb = Kb * m
where Kb is the boiling point elevation constant and m is the molality of the solution.
Given that the boiling point of the solution is 374.38°C and the boiling point elevation constant for water is 0.512 °C/m, we can rearrange the formula to solve for m:
m = ∆Tb / Kb
Substituting the given values, we get:
m = 374.38 °C / 0.512 °C/m
m ≈ 730.55 mol/kg
Next, we need to calculate the molality (m) of the solution, which is the moles of the salt per kilogram of water.
To find the moles of the salt (n), we can use the formula:
n = given mass / molar mass
The given mass of the salt is 9.18 grams. To convert grams to kilograms, divide by 1000.
n = 9.18 g / (96 g/mol)
n ≈ 0.0956 mol
Now, we can calculate the molality (m) using the following formula:
m = n / (mass of water in kg)
Given that the mass of water is 100.0 grams, we convert it to kilograms by dividing by 1000.
m = 0.0956 mol / 0.1 kg
m = 0.956 mol/kg
Having obtained the molality (m) as 0.956 mol/kg, we can compare it to the calculated molality (730.55 mol/kg) we found earlier.
It is clear that the calculated molality is significantly larger than the actual molality, suggesting that a mistake was made in the calculation.
Please double-check the given information and calculations, and provide accurate values for the boiling point of the solution, the molar mass of the metal, and the mass of water.