Based on the phase diagram of CO2 shown in Figure 11.39(b), descr...

Question

Based on the phase diagram of CO2 shown in Figure 11.39(b), describe the state changes that occur when the temperature of CO2 is increased from 190 K to 350 K at a constant pressure of (b) 5.1 atm, (c) 10 atm, and (d) 100 atm.

Accepted Answer

Step 1: Understand the phase diagram of CO2. A phase diagram shows the state of a substance (solid, liquid, gas) at various temperatures and pressures. Key points include the triple point, critical point, and the lines separating different phases.. Step 2: For (b) 5.1 atm: Locate 5.1 atm on the pressure axis of the phase diagram. At 190 K, CO2 is likely in the solid phase. As temperature increases, observe the path on the diagram to determine when CO2 transitions from solid to gas (sublimation) since 5.1 atm is below the triple point pressure.. Step 3: For (c) 10 atm: Locate 10 atm on the pressure axis. At 190 K, CO2 is in the solid phase. As temperature increases, CO2 will first transition from solid to liquid (melting) and then from liquid to gas (vaporization) as it crosses the phase boundaries.. Step 4: For (d) 100 atm: Locate 100 atm on the pressure axis. At 190 K, CO2 is in the solid phase. As temperature increases, CO2 will transition from solid to liquid (melting) and then from liquid to gas (vaporization) as it crosses the phase boundaries.. Step 5: Summarize the state changes: At 5.1 atm, CO2 sublimes from solid to gas. At 10 atm, CO2 melts from solid to liquid and then vaporizes to gas. At 100 atm, CO2 also melts from solid to liquid and then vaporizes to gas.>