If the osmotic pressure of glucose solution is 1.52 bar at 300 K. What would be its concentration if R = 0.083L bar `"mol"^(-1)"K"^(-1)` ?

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 bars at the same temperature, what would be its concentration?

The Osmotic pressure of solution containing 4.0g of solute (molar mass 246) per litre at 27^@C is (R = 0.082L atm "k"^(-1) "mol"^(-1) )

At 300K, the osmotic pressue of 300mL of a protein aqueous solution is 8.3 xx 10^(-5) bar. The molar mass of protein is 10^4 "gmol^(-1) . What is the weight (in g) of the protein present in this solution ? (R=0.083 L bar "mol"^(-1) K^(-1) )

300 mL of an aqueous solution of a protein contains 2.52 g of the protein. If osmotic pressure of such a solution at 300 K is 5.04xx10^(-3) bar, the molar mass of the protein in g mol^(-1) is

What is the value of gas constant R in J mol^(-1 ) K^(-1) ?

One mole of an ideal monoatomic gas expands isothermally against constant external pressure of 1 atm from initial volume of 1l to a state where its final pressure becomes equal to external pressure. If initial temperature of gas is 300K then total entropy change of system in the above process is: [R =0.082L atm mol^(-1)K^(-1)= 8.3J mol^(-1) K^(-1) ]

At 27^@C , one mole of an ideal gas exerted a pressure of 0.821 atmospheres. What is its volume in litres ? (R = 0.082 "lit-atm/mol"^(-1) K^(-1))

The volume occupied by 8.8 gm of CO_2 at 31.1^@C and 1 bar pressure (R = 0.083 "bar. It K"^(-1)mol^(-1)) is