Calculate the temperature of $0.05 \ M$ sucrose solution in Kelvin if the osmotic pressure of the solution is $1.5 \ atm$. $[R = 0.0821 \ dm^3 \ atm \ K^{-1} \ mol^{-1}]$

$A$ $0.6 \%$ solution of urea is isotonic with which of the following?

When $10 \ g$ of glucose (osmotic pressure $P_1$),$10 \ g$ of urea (osmotic pressure $P_2$),and $10 \ g$ of sucrose (osmotic pressure $P_3$) are dissolved in $250 \ mL$ of water,the correct relationship between the osmotic pressures of these solutions is:

If a $5.25\% \, w/v$ solution of a substance is isotonic with a $1.5\% \, w/v$ solution of urea $(Molar \, mass = 60 \, g \, mol^{-1})$ in the same solvent,then the molar mass of the substance is ........ $g \, mol^{-1}$. (in $.0$)

If a $0.1 \ M$ solution of glucose (mol. wt. $180$) and $0.1 \ M$ solution of urea (mol. wt. $60$) are placed on the two sides of a semipermeable membrane to equal heights,then it will be correct to say

$90 \, g$ of $CH_3COOH$ $(i = 0.5)$ is dissolved in $110 \, g$ of benzene. What will be its osmotic pressure at $300 \, K$ if the density of the solution is $1.2 \, g/mL$? (Answer in $atm$)