AP EAMCET · Chemistry · Solutions
\(300 \mathrm{~mL}\) of an aqueous solution of a protein contains \(2.52 \mathrm{~g}\) of the protein. If osmotic pressure of such a solution at \(300 \mathrm{~K}\) is \(5.04 \times 10^{-3}\) bar, the molar mass of the protein in \(\mathrm{g} \mathrm{mol}^{-1}\) is
- A \(83.0 \times 10^3\)
- B \(20.8 \times 10^3\)
- C \(41.5 \times 10^3\)
- D \(41.5 \times 10^4\)
Answer & Solution
Correct Answer
(C) \(41.5 \times 10^3\)
Step-by-step Solution
Detailed explanation
\(p=i \times M \times R \times T\) \[ \begin{aligned} & p=\text { osmotic pressure }=5.04 \times 10^{-3} \text { bar }=5.04 \mathrm{~atm} \\ & i=\text { van't Hoff constant }=1 \text { for undissociating } \\ & \text { molecules like protein } \end{aligned} \] molecules like…
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