If the plot is not displayed, please see Figure F13-4-2-b (the water phase diagram) in the eBook to answer this question.

Above is the phase diagram of water. What phase transition(s) can occur at a constant pressure of 10.0 atm going from T = 200 K to T = 400 K?

[Select all that apply.]

Question

If the plot is not displayed, please see Figure F13-4-2-b (the water phase diagram) in the eBook to answer this question.

Above is the phase diagram of water. What phase transition(s) can occur at a constant pressure of 10.0 atm going from T = 200 K to T = 400 K?

[Select all that apply.]

BlackTom AI · Accepted Answer

To solve this, we examine the water phase diagram at a fixed pressure of about 10 atm and track temperature from 200 K up to 400 K.

Option 1: vaporization. This would require the system to move from liquid to gas. At 10 atm, the liquid–vapor boundary (boiling line) lies at temperatures well above room temperature but well below 400 K. Since our temperature range only reaches 400 K (127°C), which is still below the typical boiling point at 10 atm (around 180°C), the system starts in a solid phase and remains below the liquid–gas boundary until temperatures near the boundary are reached; however, as we pass through the solid–liquid line first, the immediate transition encountered is solid to liquid (melting). There is no vaporization event expected within this temperature path at 10 atm.

Option 2: melting. As temperature increases at 10 atm, the solid–liquid boundary is crossed at a melting point for that pressure. For water, the solid–liquid boundary (ice Ih to liquid water) has a negative slope with pressure, so increasing pressure lowers the melting temperature slightly, but at 10 atm the melting point is still below 273 K and the system transitions from ice to liquid during heating. This is the primary phase transition along the path from 200 K to ~270 K at this pressure.

Option 3: sublimation. Sublimation is the transition from solid directly to gas. At 10 atm, the solid–gas boundary occurs at much higher temperatures than the path starting from 200 K would reach before hitting the solid–liquid boundary. Since we cross into the liquid phase before any gas-phase region is encountered, sublimation does not occur along this path.

Option 4: deposition. Deposition is the gas-to-solid transition. Since we begin as solid and heat, not cool from gas to solid, and we do not encounter a gas phase along this heating path at 10 atm, deposition is not applicable here.

Option 5: freezing. Freezing is the reverse of melting, i.e., liquid to solid. Along the described heating path from 200 K to 400 K at 10 atm, the system starts as solid and becomes liquid upon crossing the melting boundary; there is no liquid-to-solid transition during heating, so freezing does not occur.

Option 6: condensation. Condensation is gas-to-liquid. Since we are not in a gas phase at 10 atm during this heating path (we start in solid and move to liquid), condensation does not occur here.

In summary, the only phase transition that can occur at a constant pressure of 10 atm while heating from 200 K to 400 K is melting (solid to liquid) as you cross the solid–liquid boundary. The other transitions require crossing the liquid–gas or solid–gas boundaries or involve the reverse processes that do not happen along this heating trajectory at 10 atm.

CHEM 110 Section 3 (PM) SP25 Pre-Lecture 29 Quiz C13-3-5

If the plot is not displayed, please see Figure F13-4-2-b (the water phase diagram) in the eBook to answer this question. Above is the phase diagram of water. What phase transition(s) can occur at a constant pressure of 10.0 atm going from T = 200 K to T = 400 K? [Select all that apply.]

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