Equal volumes of $0.2 \ M$ urea and $0.2 \ M$ glucose are mixed. The mixture will have

Find the amount of solute in a solution obtained by dissolving it in $2.5 \ dm^3$ of water that generates an osmotic pressure of $0.245 \ atm$ at $300 \ K$. (Molar mass of solute $= 58 \ g \ mol^{-1}$,$R = 0.0821 \ dm^3 \ atm \ K^{-1} \ mol^{-1}$) (in $g$)

$18 \ g$ glucose (Molar mass $= 180 \ g/mol$) is dissolved in $100 \ mL$ of water at $300 \ K$. If $R = 0.0821 \ L \ atm \ K^{-1} \ mol^{-1}$,what is the osmotic pressure of the solution (in $atm$)?

At a constant temperature,the osmotic pressures of a $1.5 \ M \ NH_4NO_3$ aqueous solution and an $x \ M \ Al_2(SO_4)_3$ aqueous solution are approximately equal. Find the value of $x$. (Assume $100 \%$ dissociation of the solute in the solution.)

At a certain temperature,the osmotic pressure of a $0.25 \, M$ solution of a non-electrolyte is $\pi \, bar$. What will be the osmotic pressure of a $0.125 \, M \, Ba(NO_3)_2$ solution at the same temperature?

$A$ $5 \%$ solution of cane sugar (mol. wt. $= 342$) is isotonic with $1 \%$ solution of a substance $X$. The molecular weight of $X$ is