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प्रश्न
Henry's constant for \[\ce{CH3Br_{(g)}}\] is 0.159 mol dm−3 bar−1 25°C. Calculate its solubility in water at 25°C, if its partial pressure is 0.164 bar.
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उत्तर
Given:
Henry's constant for \[\ce{CH3Br_{(g)}}\] = KH = 0.159 mol dm−3 bar−1
Partial pressure (P) = 0. 164 bar
To find:
Solubility, S = ?
Formula:
S = KHP
S = 0.159 × 0.164
S = 0.02607 mol L−1
∴ Solubility of \[\ce{CH3Br_{(g)}}\] at the given condition, is 0.2607 ≅ 0.0261 mol L−1.
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