The following graph (fig. 10-7 from your textbook) displays the molar solubility of oxygen at a pressure of 1.00 atm as a function of temperature.

Question

Read the graph to determine the molar concentration of oxygen dissolved at 25 °C and 1 atm oxygen pressure. Then use Henry's law to predict the molar concentration of oxygen dissolved at 25 °C and an oxygen pressure of 5.17 atm.  ___________ M

Enter your value for molar concentration using E-notation with three significant figures.

Answer 1

My guess:

Henry's Law : C=kP

Where

C = concentration of dissolved gas (M)

k = Henry's Law constant

P = partial pressure of the gas (atm)

You have a graph that tells you the concentration of oxygen at a partial pressure of 1 atm.

From this, you will now have the concentration (C = something from the Y axis of the graph) and the partial pressure (P = 1 atm, which is what they told us it was in the graph)

You can use algebra on Henry's Law to find k: C/P = k.

Now that you have the value of k, you can use this value to find your concentration.

C = k (which you found) x 5.17 atm

And then I am assuming you know how to do scientific notation (E-notation) but let us know if you need help on that.