# Interpreting a Phase Diagram? The correct answer (that is false) is A) however can someone please explain why the other options would be true and why it is in fact possible to compress a solid to produce a liquid?

• Do you mean by reference to the provided diagram (from which all the true answers are clearly true)? As for how you compress a solid to produce a liquid, one clear answer would be that the liquid is denser than the solid forms, and thus is preferred under high enough pressure. An example is lithium. – Jon Custer Apr 15 '15 at 19:54

Let us go through this step-by-step:

1. A: A is undeniably false because if we pick a point on the solid side of the graph and add pressure to it, the point eventually becomes the liquid.

2. B: B is true because the triple point temperature is where they all intersect, and the temperature there is less than the critical point temperature.

3. C: You have to understand that C is a can question; it is true because you can form a gas or a liquid.

4. D: As you can see, where the substance changes phase is below 300 K, so we can assume that this one is also true.

5. E: The liquid will boil when the vapor pressure equals the pressure. The line from the triple point to the critical point is sloping up. So this is also true.

That leaves us with A as the only false answer.

You might want to review some concepts on phase changes and pressures.

However just to add as a side note, this question kind of seems like a homework question, you might want to add more detail and your process, so that people can take the time to answer you back. Showing some effort, gives a cause for others to care.

Thanks.

Sources: Jon Custer helped find out E.

• For E remember that the liquid will boil when it's vapor pressure equals the applied pressure. The line from the triple point to the critical point is sloping up. – Jon Custer Apr 16 '15 at 2:30
• Yup, thank you. I will add that into my answer. – Asker123 Apr 16 '15 at 19:51