Chemical Forums
Chemistry Forums for Students => High School Chemistry Forum => Topic started by: kdbmvp on February 21, 2019, 05:25:48 AM
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Hello,
How much N2 can be solved in 1L of water at 20 celsius, 1 atm total pressure, if the partial pressure of the N2 gas is 0.78atm? From a table I found that the solubility of N2 in water at 20 celsius is 0.0190 g/L, at a total pressure of 1 atm. The solution manual calculates it this way:
0.78atm*0.0190 g/L = 0.01482 g/L. But is this correct? From how I understand the task the answer should just be 0.0190 g/L
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What does this "total pressure" mean? If it's 1atm of air, then 0.78atm of N2 is reasonable. If it's 1atm of N2, you need to scale down to 0.78atm.
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Total pressure was probably the wrong word. It just says: how much N2 can be solved in 1L of water at 20 celsius and 1 atm pressure. Not sure if I entirely understood your answer?
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Total pressure was probably the wrong word. It just says: how much N2 can be solved in 1L of water at 20 celsius and 1 atm pressure. Not sure if I entirely understood your answer?
Amount of nitrogen dissolved will depend on the partial pressure of nitrogen, other gases don't matter (or rather: effect of their presence ins negligible). What is the partial pressure of nitrogen?
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The partial pressure of N2 is 0.78 atm
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As Enthalpy wrote: assuming the data given was solubility for 1 atm of nitrogen, you should scale the solubility to 0.78 atm (remembering what Henry's law says).