What is the relationship between delta T and molar mass of solute?
The larger the value of delta T, the (larger,smaller) the molar mass of the solute?
delta T = Kf*m
m = moles/kg solvent
moles = grams/molar mass.
The above three equations will answer the second part.
I need help
The molar mass of the solute is indirectly proportional to the value of delta T. This means that as the value of delta T increases, the molar mass of the solute decreases. So, the correct answer is "smaller" - the larger the value of delta T, the smaller the molar mass of the solute.
To determine the relationship between delta T (change in temperature) and the molar mass of a solute, we need to understand colligative properties and the concept of boiling point elevation or freezing point depression.
Colligative properties are properties that depend on the number of particles (molecules or ions) in a solution, rather than the chemical nature of those particles. Boiling point elevation and freezing point depression are colligative properties, which means they depend on the number of solute particles present.
The relationship between delta T and the molar mass of a solute can be explained using the following equation:
delta T = K * m * i
where:
- delta T is the change in temperature of a solution
- K is the molal boiling point elevation or freezing point depression constant (specific for a particular solvent)
- m is the molality of the solute (moles of solute per kilogram of solvent)
- i is the van 't Hoff factor, which represents the number of particles the solute dissociates into (e.g. ions) when dissolved in the solvent
According to the equation, delta T is directly proportional to the molality of the solute (m) and the van 't Hoff factor (i). This means that as the molality of the solute or the number of dissolved particles increases, delta T will also increase.
However, there is no direct relationship between delta T and the molar mass of the solute. The molar mass only indirectly affects delta T through its influence on the number of moles of the solute in a given mass of the solution. The van 't Hoff factor (i) depends on the nature of the solute, not its molar mass.
Therefore, we cannot conclude that a larger delta T always corresponds to a larger or smaller molar mass of the solute. The relationship between them depends on the specific solute and its ability to dissociate into multiple particles in the solvent.