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

Henry's law is the kP_i = C_i or that the concentration of a gas in a liquid is directly proportional to its partial pressure. The easiest way to do this is to find the P_O2 at 1 atm off of the chart:

C(P₂) = C(P₁)(P₂/P₁) and, in this case P₁ = 1 atm, so you are just multiplying the concentration by the number of atmospheres at the new pressure.