The normal melting and boiling point of O2 are -218C and 49.8atm. a)Sketch the phase diagram for O2. b) Which is denser, O2(S) or O2 (l)? explain.
49.8 atm is not a boiling point. It is a pressure (50.4 atm is what is called the critical pressure of O2; that may be what you meant to write). The boiling point of O2 is -183 C
http://www.fileden.com/files/2006/8/29/193519/PD%20of%20O2.jpg
shows you the phase diagram of O2
thanks, i typed it wrong
Is it O2(S) is denser right? Because it's solid
To answer the first part of your question, we can sketch the phase diagram for O2 (oxygen). Here's how you can do it step by step:
Step 1: Determine the temperature and pressure range. The given information tells us that the normal melting point of O2 is -218°C, and the normal boiling point is -183°C.
Step 2: Plot the temperature on the horizontal axis. Choose a suitably large range of temperatures that include the melting and boiling points. In this case, let's say from -250°C to -150°C.
Step 3: Plot the pressure on the vertical axis. Again, choose a suitable range of pressures. Since the given boiling point is at 49.8 atm, we can choose a range from 0 atm to 60 atm.
Step 4: Mark the triple point. The triple point is the unique combination of temperature and pressure at which all three phases (solid, liquid, and gas) can coexist in equilibrium. In this case, the triple point for O2 is at -218°C and 49.8 atm. Mark this point on the diagram.
Step 5: Draw the phase boundaries. Connect the triple point to the melting point and the boiling point with lines. The line connecting the triple point to the melting point represents the solid-liquid phase boundary. The line connecting the triple point to the boiling point represents the liquid-gas phase boundary.
Step 6: Label the phases. At temperatures below the melting point, O2 is a solid (O2 (s)). Between the melting and boiling points, it is a liquid (O2 (l)). At temperatures above the boiling point, it is a gas (O2 (g)). Label each phase accordingly.
Now, to answer the second part of your question. The denser phase of O2 is the liquid phase (O2 (l)). When a substance melts, it usually undergoes a volume expansion. However, when a substance undergoes a phase change from a liquid to a gas (boiling), it undergoes a significant volume increase. This means that the gas phase of O2 (O2 (g)) is less dense than the liquid phase (O2 (l)). So, O2 (l) is denser than O2 (g).