It’s Calcium hope that helps!
Answer:
Molar mass of unknown solute is 679 g/mol
Explanation:
Let us assume that the solute is a non-electrolyte.
For a solution with non-electrolyte solute remains dissolved in it -
Depression in freezing point of solution, ![\Delta T_{f}=K_{f}.m](https://tex.z-dn.net/?f=%5CDelta%20T_%7Bf%7D%3DK_%7Bf%7D.m)
where, m is molality of solute in solution and
is cryogenoscopic constant of solvent.
Here ![\Delta T_{f}=(-22.9^{0}\textrm{C})-(-28.7^{0}\textrm{C})=5.8^{0}\textrm{C}](https://tex.z-dn.net/?f=%5CDelta%20T_%7Bf%7D%3D%28-22.9%5E%7B0%7D%5Ctextrm%7BC%7D%29-%28-28.7%5E%7B0%7D%5Ctextrm%7BC%7D%29%3D5.8%5E%7B0%7D%5Ctextrm%7BC%7D)
If molar mass of unknown solute is M g/mol then-
![m=\frac{\frac{2.2}{M}}{0.0167}mol/kg](https://tex.z-dn.net/?f=m%3D%5Cfrac%7B%5Cfrac%7B2.2%7D%7BM%7D%7D%7B0.0167%7Dmol%2Fkg)
So, ![5.8^{0}\textrm{C}=29.9^{0}\textrm{C}/(mol/kg)\times \frac{\frac{2.2g}{M}}{0.0167}mol/kg](https://tex.z-dn.net/?f=5.8%5E%7B0%7D%5Ctextrm%7BC%7D%3D29.9%5E%7B0%7D%5Ctextrm%7BC%7D%2F%28mol%2Fkg%29%5Ctimes%20%5Cfrac%7B%5Cfrac%7B2.2g%7D%7BM%7D%7D%7B0.0167%7Dmol%2Fkg)
so, M = 679 g/mol
Answer: A sea of electrons
Explanation: