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The concentration of N2 in the ocean at 25∘C is 445μM. The Henry's law constant for N2 is 0.61×10−3 molL−1atm−1.

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The concentration of N2 in the ocean at 25∘C is 445μM. The Henry's law constant for N2 is 0.61×10−3 molL−1atm−1.

Post  John Lord on Fri Feb 13, 2015 1:18 pm

The concentration of N2 in the ocean at 25∘C is 445μM. The Henry's law constant for N2 is 0.61×10−3 molL−1atm−1.

Part A)

Calculate the mass of N2 in a liter of ocean water.
Express your answer to three significant figures and include the appropriate units.

The correct answer is; however, I do not have an idea how it was calculated.

m = 1.25×10−2 gL

Part B)

Calculate the partial pressure of N2 in the atmosphere.
Express your answer to two significant figures and include the appropriate units. (I do not know how to go about solving this question)

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Conc N2 in ocean water & Partial pressure N2 in atm.

Post  DrPelezo on Fri May 22, 2015 5:52 pm

To solve this problem you need to understand what a micro-molar solution is, and convert it to a molar solution = moles N2/Liter Ocean Water. Then multiply by the formula wt of N2 . Working from the 445-μM concentration as suggested, you will get the 1.25 x 10-2 g/L. However, working from the Henry's Law equation, Solubility(mol/L) = k x Applied Pressure(atm.) & using the Henry's Law constant as given, calculates Solubility N2(g) = 1.72 x 10-2 g/L.

To determine the partial pressure of N2 (g) in the atmosphere, Assume the atmospheric total pressure is 760-mmHg and that %N2(g) is 79% by wt. That means 79% of the atm pressure is the partial pressure of nitrogen gas. ( P(N2) = 600.4 mmHg. )


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