how do you find the boiling temp of 2m of c6h12o6
in water?
delta T = Kb*m. Solve for delta T and add to 100 C.
To find the boiling temperature of a solution, you need to know the boiling point elevation constant (Kb) and the molality of the solute.
Step 1: Determine the molality of the solute (C6H12O6) in the solution.
- Molality (m) is calculated by dividing the moles of solute by the mass of the solvent.
- Since you mentioned that there are 2m of C6H12O6, we need to convert it to moles.
- The molar mass of C6H12O6 (glucose) is approximately 180.16 g/mol.
- Therefore, the moles of C6H12O6 can be calculated by dividing the mass by its molar mass.
Step 2: Determine the boiling point elevation constant (Kb).
- The Kb value is specific to the solvent used. Since you haven't mentioned the solvent, I cannot provide you with the exact Kb value.
- Common Kb values for different solvents can be found in literature or online.
Step 3: Calculate the boiling point elevation (∆Tb) using the molality (m) and the Kb value.
- The boiling point elevation can be calculated using the formula: ∆Tb = Kb * m.
- This formula only holds for dilute solutions where the molality is not too high.
Step 4: Calculate the boiling temperature (Tb) of the solution.
- The boiling temperature (Tb) of the solution is calculated by adding the boiling point elevation (∆Tb) to the boiling point of the pure solvent.
- The boiling point of the pure solvent can also be found in literature or online.
Keep in mind that this calculation assumes ideal conditions and is based on the assumption that the solute does not dissociate or interact with the solvent in a non-ideal way. It also assumes that the solution is dilute enough for the formula to be valid.
Please provide the solvent and the boiling point elevation constant to get a more accurate calculation.
To find the boiling point of a substance, such as C6H12O6 (glucose), you need to know the boiling point elevation constant and the molality of the solution.
The boiling point elevation constant, Kb, is a property of the solvent and can be found in reference books or online. For water (the solvent in this case), the Kb value is approximately 0.51 °C/m.
To calculate the boiling point elevation, you need to know the molality (moles of solute per kilogram of solvent) of the solution. Since you have the mass of C6H12O6 (glucose) and its molar mass, you can calculate the number of moles, and then divide it by the mass of water (assuming water is the solvent) to find the molality.
Once you have the molality, you can use the following formula to calculate the boiling point elevation:
ΔTb = Kb * molality
In this case, substituting the values, you can calculate the boiling point elevation, ΔTb, which is the difference between the boiling temperature of the solution and the boiling temperature of the pure solvent (water).
Finally, to find the boiling temperature, you need to add the calculated boiling point elevation to the boiling temperature of pure water, which is 100 °C at standard atmospheric pressure.
It's important to note that this method assumes ideal behavior and takes into account the colligative properties of solutions, which are properties that depend on the number of solute particles rather than their identity.