The presence of the radioactive gas radon (Rn) in well water presents a possible health hazard in parts of the United States. (a) Assuming that the solubility of radon in water with 1 atm pressure of the gas over the water at 30 °C is 7.27⨉10^-3 M, what is the Henry's law constant for radon in water at this temperature?

Question

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Hello everyone today. We have been given the following problem and ask her to solve for it. It says carbon monoxide is one of the toxic substances that can be found in water. Carbon monoxide has a cell viability of 9.85 times 10 to the negative fourth polarity at 25 degrees Celsius 1 80 M. Or one atmospheres were then asked to calculate Henry's law constant for carbon monoxide in water. So the first thing we wanna do is you want to write the formula for this law. That formula will say that we have our concentration of dissolved gas, which in this case will be our carbon monoxide. We're going to equal that to Henry's law constant or K. And that's gonna be multiplied by the partial pressure of our gas, which is carbon monoxide rearranging this equation to solve for K. We get K. Is equal to our concentration of our carbon monoxide over our partial pressure of that carbon monoxide. Let me simply plug in our values So our concentration of our dissolved gas, which is carbon monoxide is going to be 9.85 times 10 to the negative fourth polarity. And the partial pressure is going to be one atmospheres. And so that leaves us with a constant of 9. times 10 to the negative fourth moles over leaders times atmospheres as our units. And this is our final answer. I hope this helped. And until next time

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Key Concepts

Henry's Law

Solubility

Units of Henry's Law Constant