The Henry's law constant for oxygen is $1 \cdot 3 \times 10^{-3} \mathrm{~mol} \mathrm{dm}^{-3}…

The Henry's law constant for oxygen is $1 \cdot 3 \times 10^{-3} \mathrm{~mol} \mathrm{dm}^{-3} \mathrm{~atm}^{-1}$. If partial pressure of oxygen is $0.46$ atmosphere what is the concentration of dissolved oxygen at $25^{\circ} \mathrm{C}$ and 1 atm pressure?
  1. $5.98 \times 10^{-4} \mathrm{~mol} \mathrm{dm}^{-3}$
  2. $3.53 \times 10^{-4} \mathrm{~mol} \mathrm{dm}^{-3}$
  3. $5.98 \mathrm{~mol} \mathrm{dm}^{-3}$
  4. $2 \cdot 82 \times 10^{-3} \mathrm{~mol} \mathrm{dm}^{-3}$

Solution

$\mathrm{K}_{\mathrm{H}}=\frac{\mathrm{S}}{\mathrm{P}} \quad \therefore \mathrm{S}=\mathrm{K}_{\mathrm{H}} \times \mathrm{P}$ $\therefore \mathrm{S}=1.3 \times 10^{-3} \mathrm{~mol} \mathrm{dm}^{-3} \mathrm{~atm}^{-1} \times 0.46 \mathrm{~atm}=5.98 \times 10^{-4} \mathrm{~mol} \mathrm{dm}^{3}$

Asked in: MHT CET 2020 (12 Oct Shift 2)

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