Find the mass of urea needed to prepare 51.7 g of a solution in water in which the mole fraction of urea is 7.59×10−2. anyone have the same values?
To find the mass of urea needed to prepare the given solution, we need to use the mole fraction and the molar mass of urea.
First, let's calculate the number of moles of urea in the solution. We can do this by multiplying the mole fraction of urea by the total number of moles in the solution.
Number of moles of urea = Mole fraction of urea * Total moles in the solution
The total moles in the solution can be calculated using the formula:
Total moles in the solution = Mass of solution / Molar mass of solvent
In this case, since urea is the solute, water is the solvent. The molar mass of water is approximately 18 g/mol.
Mass of solution = 51.7 g
Molar mass of solvent (water) = 18 g/mol
Total moles in the solution = 51.7 g / 18 g/mol
Now, we can substitute the values to calculate the number of moles of urea:
Number of moles of urea = 7.59×10−2 * (51.7 g / 18 g/mol)
Next, we need to find the molar mass of urea. The molar mass of urea is approximately 60 g/mol.
Now we can calculate the mass of urea needed:
Mass of urea = Number of moles of urea * Molar mass of urea
Mass of urea = (7.59×10−2 * (51.7 g / 18 g/mol)) * 60 g/mol
By calculating the above expression, we can find the mass of urea needed to prepare the given solution.