Calculate the osmotic pressure of a solution containing $0.025 \ mol$ of glucose in $100 \ mL$ of water at $300 \ K$. $\left[R = 0.082 \ atm \ dm^3 \ mol^{-1} \ K^{-1}\right]$ (in $atm$)

Which one of the following pairs of solutions can we expect to be isotonic at the same temperature?

$A$ solution of a non-electrolyte substance containing $1.05 \ g$ per $100 \ mL$ was found to be isotonic with a $3\%$ glucose solution. The molecular mass of the substance is:

The osmotic pressure of $1 \, M$ solution at $27 \, ^\circ C$ is ........... $atm$.

$A$ solution containing $10 \ g/L$ of urea is isotonic with a $5\%$ solution of a non-electrolyte solute. The molecular mass of the non-electrolyte solute is ..... $g/mol$.

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 $M$)?