The molality of aqueous urea solution is 1.2m the the mole fraction of urea in aqueous solution is

To find the mole fraction of urea in the aqueous solution, we first need to understand the definitions of molality and mole fraction.

1. Molality (m) is defined as the number of moles of solute (in this case, urea) per kilogram of solvent (in this case, water). In this problem, the molality of the urea solution is given as 1.2m, which means there are 1.2 moles of urea per kilogram of water.

2. Mole fraction is defined as the ratio of the number of moles of a component to the total number of moles of all components in the solution.

Step 1: Calculate the moles of water Since the density of water is approximately 1g/mL, 1 kilogram of water is approximately 1000g or 1000mL. The molar mass of water is approximately 18g/mol, so there are approximately 1000g / 18g/mol = 55.56 moles of water in 1 kilogram.

Step 2: Calculate the total moles in the solution The total number of moles in the solution is the sum of the moles of urea and the moles of water. So, total moles = 1.2 moles (urea) + 55.56 moles (water) = 56.76 moles.

Step 3: Calculate the mole fraction of urea The mole fraction of urea is the number of moles of urea divided by the total number of moles in the solution. So, mole fraction of urea = 1.2 moles / 56.76 moles = 0.0211.

So, the mole fraction of urea in the aqueous solution is approximately 0.0211.