Question

Calculate the dissolved oxygen in mg/L at an altitude of 1,000 m above sea level that has an atmospheric pressure of 0.89 atm, assuming a constant temperature of 25 °C. The Henry's Law constant (kH) for the solubility of O2 in water at 25 °C is 1.3 x 10-3 mol/L.atm.

Name: calculate the dissolved oxygen in mgl at an altitude of 1000 m above sea level that has an atmospheric pressure of 089 atm assuming constant temperature of 25 c the henry law constant kh for 33878
Uploaded: 2022-06-14T19:35:06-08:00
Duration: 2 min 4 s
Channel: David Collins
Description: calculate the dissolved oxygen in mgl at an altitude of 1000 m above sea level that has an atmospheric pressure of 089 atm assuming constant temperature of 25 c the henry law constant kh for 33878

          Calculate the dissolved oxygen in mg/L at an altitude of 1,000 m above sea level that has an atmospheric pressure of 0.89 atm, assuming a constant temperature of 25 °C. The Henry's Law constant (kH) for the solubility of O2 in water at 25 °C is 1.3 x 10-3 mol/L.atm.

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Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert David Collins

06/14/2022

Step 1

Given: Henry's Law constant (kH) = 1.3 x 10^-3 mol/L.atm Pressure (P) = 0.89 atm Concentration of oxygen = kH * P Concentration of oxygen = 1.3 x 10^-3 mol/L.atm * 0.89 atm Concentration of oxygen = 1.157 x 10^-3 mol/L Show more…

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Calculate the dissolved oxygen in mg/L at an altitude of 1,000 m above sea level that has an atmospheric pressure of 0.89 atm, assuming a constant temperature of 25 °C. The Henry's Law constant (kH) for the solubility of O2 in water at 25 °C is 1.3 x 10-3 mol/L.atm.