Solutions having the same osmotic pressure under a given set of conditions are known as

The relationship between osmotic pressure at $273 \ K$ when $10 \ g$ glucose $(P_1)$,$10 \ g$ urea $(P_2)$,and $10 \ g$ sucrose $(P_3)$ are dissolved in $250 \ mL$ of water is:

$50 \ mL$ of $0.2$ molal urea solution (density $= 1.012 \ g \ mL^{-1}$ at $300 \ K$) is mixed with $250 \ mL$ of a solution containing $0.06 \ g$ of urea. Both the solutions were prepared in the same solvent. The osmotic pressure (in Torr) of the resulting solution at $300 \ K$ is . . . . . $[\Delta_{mix} V = 0]$

Which statement is wrong regarding osmotic pressure $P$,volume $V$,and temperature $T$?

The osmotic pressure (in $atm$) of an aqueous solution containing $0.01 \ mol$ of $NaCl$ (degree of dissociation $0.94$) and $0.03 \ mol$ of glucose in $500 \ mL$ at $27^{\circ} C$ is $\left(R=0.082 \ L \ atm \ K^{-1} \ mol^{-1}\right)$

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