Question

100 ml of a glucose solution at 298 K
has osmotic pressure 6.1 atm. Hence the
mass of glucose present in solution is

Answer 1

Answer:

Answer : The moles of glucose dissolved per liter of solution will be, 0.11 moles

Solution : Given,

Osmotic pressure = 2.72 atm

Temperature = 298 K

Formula used :

$$\begin{lgathered}\pi=iCRT\\\\C=\frac{\pi}{iRT}\end{lgathered}$$

where,

$$\pi$$ = osmotic pressure

i = van't Hoff factor of glucose = 1

C = concentration of solution

R = Gas constant = 0.0821 Latm/moleK

T = temperature

Now put all the given values in the above formula, we get

$$C=\frac{2.72atm}{1\times (0.0821Latm/moleK)\times (298K)}=0.11mole/L$$

Therefore, the moles of glucose dissolved per liter of solution will be, 0.11 molesAnswer : The moles of glucose dissolved per liter of solution will be, 0.11 moles

Solution : Given,

Osmotic pressure = 2.72 atm

Temperature = 298 K

Formula used :

$$\begin{lgathered}\pi=iCRT\\\\C=\frac{\pi}{iRT}\end{lgathered}$$

where,

$$\pi$$ = osmotic pressure

i = van't Hoff factor of glucose = 1

C = concentration of solution

R = Gas constant = 0.0821 Latm/moleK

T = temperature

Now put all the given values in the above formula, we get

$$C=\frac{2.72atm}{1\times (0.0821Latm/moleK)\times (298K)}=0.11mole/L$$

Therefore, the moles of glucose dissolved per liter of solution will be, 0.11 moles

Explanation:

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