$0.2 \ M$ aqueous solution of glucose has osmotic pressure $4.9 \ atm$ at $300 \ K$. What is the concentration of glucose if it has osmotic pressure $1.5 \ atm$ at same temperature (in $M$)?

$A$ solution containing $4 \ g$ of a non-volatile organic solute per $100 \ mL$ has an osmotic pressure of $500 \ cm$ of mercury at $27^\circ C$. What is the molar mass of the solute?

At $300 \ K$,the osmotic pressure of a solution containing $36 \ g$ of glucose per liter is $4.98 \ bar$. If the osmotic pressure of the solution is $1.52 \ bar$ at the same temperature,what will be its concentration (in $M$)?

At $300 \, K$,$36 \, g$ of glucose present in a litre of its solution has an osmotic pressure of $4.98 \, bar$. If the osmotic pressure of the solution is $1.52 \, bar$ at the same temperature,what would be its concentration?

Consider the following pairs of solutions which will be isotonic at the same temperature. The number of pairs of solutions that are isotonic is/are..........
$A.$ $1 \ M$ aq. $NaCl$ and $2 \ M$ aq. Urea
$B.$ $1 \ M$ aq. $CaCl_2$ and $1.5 \ M$ aq. $KCl$
$C.$ $1.5 \ M$ aq. $AlCl_3$ and $2 \ M$ aq. $Na_2SO_4$
$D.$ $2.5 \ M$ aq. $KCl$ and $1 \ M$ aq. $Al_2(SO_4)_3$

If $5\%$ sugar solution is isotonic with $1\%$ solution of unknown substance,then find out the molecular mass of the unknown substance. (in $g/mol$)