How many gram of glucose when dissolved ...

How many gram of glucose when dissolved in 2 litre of water will be isotonic with blood at `37^@C`? `[pi_(blood)=7.65` atm, Molar mass of glucose=180g `mol^(1)`, R=0.082L atm `K^(-1) mol^(-1)`]

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How many gram of glucose when dissolved in 2 litre of water will be isotonic with blood at 37^(@)C ? [ pi_(blood) =7.65 atm, Molar mass of glucose = 180g mol^(-1) , R = 0.082 L . Atm. K^(-1). mol ]

10g of an organic substance when dissolved in two litres of water gave an osmotic pressure of 0.59 atm, at 7^(@)C . Calculate the molecular weight of the substance.

What is meant by the molarity of a solution ? What would be the osmotic pressure of a 0.02 molar aqueous solution of urea at 27^(@)C ? (R = 0.082 L.atm.K^(-1). Mol^(-1) )

Calculate the osmotic pressure of a 10%. Solution of glucose at 18^@C . R = 0.082 lit atm K^-1 mol^-1 .

A gas of molar mass 84.5 g//mol is enclosed in a flask at 27^@C has a pressure of 2 atm. Calculate the density of the gas. [R = 0.082 L atm K^(-1) mol^(-1)]

Calculate the freezing point of an aqueous solution of a non-electrolyte having an osmotic pressure 2.0 atm at "300 K. Kf = 1.86 k.kg.mol"^(-1.)" R = 0.0821 lit.atm.k"^(-1)" mol"^(-1)

1.19g of volatile liquid gas on complete vaporisation gives 216ml of its vapour at 27^(@) and 755 mm pressure. Calculate molar mass of liquid. (R=0.082litatmK^(-)mol^(-))

A gas of molar mass 84.5g/mol is enclosed in a flask at 27^(@)C has a pressure of 2 atm. Calculate the density of the gas. [R=0.082 *atm*K^(-1)*mol^(-1) ]

What is the freezing point of solution containing 3g of a non-volatile solute in 20g of water. Freezing point of pure water is 273K, K_(f) of water = 1.86 Kkg/mol. Molar mass of solute is 300 g/mol. T^(@)-T=K_(f)m

The mass of a copper coin is 3.2 g. suppose it was pure copper. How many moles of Cu atoms would the coin contain, given a molar mass of Cu of 63.54 g mol^(-1) ?

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