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mauvefish365Lv1
28 Sep 2019
<p>The concentration of Ar in the ocean at 25 Celsius is11.5<em>m</em>M. The Henry's law constant for Ar is 1.5X 10^3 mol X L^- 1 atm^- 1.<br /><br />Calculate themass of Ar in a liter of ocean water.</p>
<p><em>m </em>=<br /><br />Calculatethe partial pressure of Ar in the atmosphere.</p>
<p>P =</p>
<p>The concentration of Ar in the ocean at 25 Celsius is11.5<em>m</em>M. The Henry's law constant for Ar is 1.5X 10^3 mol X L^- 1 atm^- 1.<br /><br />Calculate themass of Ar in a liter of ocean water.</p>
<p><em>m </em>=<br /><br />Calculatethe partial pressure of Ar in the atmosphere.</p>
<p>P =</p>
<p><em>m </em>=<br /><br />Calculatethe partial pressure of Ar in the atmosphere.</p>
<p>P =</p>
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Keith LeannonLv2
28 Sep 2019
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Related questions
An evacuated 1.000 L flask was filled at room temperature with 4.920E-2 mol NO (nitrogen monoxide) and 7.74E-3 mol Br2 (bromine). The temperature was then raised to 50.5°C, and these substances reacted to give nitrosyl bromide, NOBr:
2NO(g) + Br(g) <--> 2NOBr(g)
When equilibrium was achieved, the pressure of the gases in the flask was found to be 1.315 atm.
(a) What was the total moles of gases in the flask at equilibrium? | ntotal = mol |
(b) How many moles of nitrosyl bromide were formed? What was the moles of each substance in the flask at equilibrium? | n(NO) = mol n(Br2) = mol n(NOBr) = mol |
(c) What are the partial pressures of the different gases in this equilibrium mixture? | p(NO) = atm p(Br2) = atm p(NOBr) = atm |
(d) What is Kp at this temperature? | Kp = |