Average osmotic pressure of human blood is $7.4 a t m$ at $27^{o} C$ , then total concentration of various solutes is:

0.1 m o l L^{- 1}

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0.2 m o l L^{- 1}

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0.3 m o l L^{- 1}

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0.4 m o l L^{- 1}

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Solution

The correct option is B $0.3 m o l L^{- 1}$
$C_{g l u c o s e} = \frac{π}{i R T}$
$C_{g l u c o s e} = \frac{7.4 a t m}{1 \times 0.0821 \frac{a t m L}{m o l k} \times (273.15 + 25) k}$
$C_{g l u c o s e} = 0.3 m o l L^{-}$

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Similar questions

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Average osmotic pressure of human blood is 7.4 atm at 27oC, then total concentration of various solutes is:

The correct option is B 0.3 molL−1Cglucose=πiRTCglucose=7.4atm1×0.0821atmLmolk×(273.15+25)kCglucose=0.3molL−

Average osmotic pressure of human blood is $7.4 a t m$ at $27^{o} C$ , then total concentration of various solutes is:

The correct option is B $0.3 m o l L^{- 1}$
$C_{g l u c o s e} = \frac{π}{i R T}$
$C_{g l u c o s e} = \frac{7.4 a t m}{1 \times 0.0821 \frac{a t m L}{m o l k} \times (273.15 + 25) k}$
$C_{g l u c o s e} = 0.3 m o l L^{-}$