Question

Find the boiling point of a solution of 92.1g of iodine, I2 in 800.0g of chloroform, CHCL3, assuming that the iodine is nonvolatile and that the solution is ideal.

Answer 1

62.91 *C

Step-by-step explanation:

Note that our solute in this example is I2 and our solvent is chloroform.

1) Convert grams to moles of I2 using Molar Mass: 92.1/253.8=0.363moles

2) Find molality from the number of moles of solute by the mass of solvent in kg.

m (molality)= (moles solute)/(Kg solvent) => 0.363/0.8=0.454m

3) Use the change in boiling point and molality of the solution to calculate how much-boiling point (Bp) changed. The Bp of chloroform is constant, and you must search online for the exact number. In this case, the Bp constant of chloroform is 3.63*C/m: m (molality)*Bp => 0.454*3.63=1.65*C

4) Finding the new Bp from the Bp of chloroform by using the change Bp in step 3. The Bp of chloroform under 1atm is 61.26*C (you must also look this one up):

61.26+1.65=62.91*C

Hope this helps!