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Calculate oxygen molar concentration in water at 25°C with a partial p
Chapter 12, Problem 12.6(choose chapter or problem)
Calculate the molar concentration of oxygen in water at \(25^{\circ}\rm{C}\) for a partial pressure of 0.22 atm. The Henry’s law constant for oxygen is \(1.3 \times 10^{-3} \ \rm{mol/L} \cdot \rm{atm}\).
Questions & Answers
QUESTION:
Calculate the molar concentration of oxygen in water at \(25^{\circ}\rm{C}\) for a partial pressure of 0.22 atm. The Henry’s law constant for oxygen is \(1.3 \times 10^{-3} \ \rm{mol/L} \cdot \rm{atm}\).
ANSWER:Step 1 of 2
Partial pressure of the system is: p=0.22 atm.
Henry’s law constant for the oxygen is: \(k=1.3 \times 10^{-3} \ \rm{mol/L} \cdot \rm{atm}\)
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Calculate oxygen molar concentration in water at 25°C with a partial p
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This video explores molar concentration (molarity) and demonstrates the calculation of oxygen's molar concentration in water at 25°C, considering a partial pressure of 0.22 atm by employing Henry's Law and the given Henry's Law constant for oxygen, revealing that under these conditions, there are 2.86 x 10?? moles of oxygen per liter of water, highlighting the significance of understanding these concepts for managing gas dissolution in liquids across varying circumstances.