Which one of the following is the incorrect form of Raoult's law?

What weight of glucose must be dissolved in $100 \ g$ of water to lower the vapour pressure by $0.20 \ mm \ Hg$ (in $g$)? (Assume dilute solution is being formed) Given: Vapour pressure of pure water is $54.2 \ mm \ Hg$ at room temperature. Molar mass of glucose is $180 \ g \ mol^{-1}$

"Relative lowering in vapour pressure of a solution containing a non-volatile solute is directly proportional to the mole fraction of the solute". The above statement is:

The vapour pressure of water at $23^{\circ} C$ is $19.8 \ mm$. If $0.1 \ mole$ of glucose is dissolved in $178.2 \ g$ of water, what is the vapour pressure (in $mm$) of the resultant solution?

Vapour pressure of pure water at $298 \, K$ is $23.8 \, mm \, Hg$. $50 \, g$ of urea $(NH_2CONH_2)$ is dissolved in $850 \, g$ of water. Calculate the vapour pressure of water for this solution and its relative lowering.

At $300 \ K$,the vapour pressure of an ideal solution containing $3 \ mol$ of $A$ and $2 \ mol$ of $B$ is $600 \ torr$. At the same temperature,if $1.5 \ mol$ of $A$ and $0.5 \ mol$ of $C$ (non-volatile) are added to this solution,the vapour pressure of the solution increases by $30 \ torr$. What is the value of $p_B^o$?