Answer : The molal freezing point depression constant of X is ![4.12^oC/m](https://tex.z-dn.net/?f=4.12%5EoC%2Fm)
Explanation : Given,
Mass of urea (solute) = 5.90 g
Mass of X liquid (solvent) = 450.0 g
Molar mass of urea = 60 g/mole
Formula used :
![\Delta T_f=i\times K_f\times m\\\\T^o-T_s=i\times K_f\times\frac{\text{Mass of urea}\times 1000}{\text{Molar mass of urea}\times \text{Mass of X liquid}}](https://tex.z-dn.net/?f=%5CDelta%20T_f%3Di%5Ctimes%20K_f%5Ctimes%20m%5C%5C%5C%5CT%5Eo-T_s%3Di%5Ctimes%20K_f%5Ctimes%5Cfrac%7B%5Ctext%7BMass%20of%20urea%7D%5Ctimes%201000%7D%7B%5Ctext%7BMolar%20mass%20of%20urea%7D%5Ctimes%20%5Ctext%7BMass%20of%20X%20liquid%7D%7D)
where,
= change in freezing point
= freezing point of solution = ![-0.5^oC](https://tex.z-dn.net/?f=-0.5%5EoC)
= freezing point of liquid X= ![0.4^oC](https://tex.z-dn.net/?f=0.4%5EoC)
i = Van't Hoff factor = 1 (for non-electrolyte)
= molal freezing point depression constant of X = ?
m = molality
Now put all the given values in this formula, we get
![[0.4-(-0.5)]^oC=1\times k_f\times \frac{5.90g\times 1000}{60g/mol\times 450.0g}](https://tex.z-dn.net/?f=%5B0.4-%28-0.5%29%5D%5EoC%3D1%5Ctimes%20k_f%5Ctimes%20%5Cfrac%7B5.90g%5Ctimes%201000%7D%7B60g%2Fmol%5Ctimes%20450.0g%7D)
![k_f=4.12^oC/m](https://tex.z-dn.net/?f=k_f%3D4.12%5EoC%2Fm)
Therefore, the molal freezing point depression constant of X is ![4.12^oC/m](https://tex.z-dn.net/?f=4.12%5EoC%2Fm)
I think it is b..................................................
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Explanation:
Answer:
will have a greater partial charge.
Explanation:
A polar covalent bond is defined as the bond which is formed when there is a low difference of electronegativities between the atoms, thus resulting in charge difference. Example: ![ClF](https://tex.z-dn.net/?f=ClF)
Non-polar covalent bond is defined as the bond which is formed when there is no difference of electronegativities between the atoms and thus there is no charge difference. Example: ![F_2](https://tex.z-dn.net/?f=F_2)
Ionic bond is formed when there is complete transfer of electron from a highly electropositive metal to a highly electronegative non metal. The electronegative difference between the elements is high. The charges on cation and anion neutralise each other. Example: ![LiCl](https://tex.z-dn.net/?f=LiCl)
Thus as
will have greater partial charge.