Posted by **Becca** on Saturday, February 4, 2012 at 8:15pm.

At a certain temperature, the solubility of N_2 gas in water at 2.38 atm is 56.0 mg of N_2 gas/100 g of water. Calculate the solubility of N_2 gas in water, at the same temperature, if the partial pressure of N_2 gas over the solution is increased from 2.38 atm to 5.00 atm.

- Chemistry -
**DrBob222**, Saturday, February 4, 2012 at 8:31pm
56 mg/100 mL = 560 mg/L = 0.560 g/L

Convert to mol/L = M = 0.560/molar mass N2.

partial pressure = kC

k = p/c = 2.38 atm/M of N2

moles N2 = 56 g/molar mass N2.

Find k, then use

p = kC, substitute 5.00 for p and k from above, solve for M N2 at 5.00 atm. The author of the problem may want you to show moles in the 100 mL so you may need to convert M to that.

- Chemistry -
**Jennifer Julizar**, Thursday, September 20, 2012 at 5:59pm
118

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