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Asked by Abhigna Last Modified
Answer To determine if CO2(g) can be liquefied at 32°C and 80 atm pressure, we need to compare the given conditions with the critical temperature (Tc) and critical pressure (Pc) of CO2.
The critical temperature (Tc) of CO2 is 30.98°C, and the critical pressure (Pc) is 73 atm.
Given conditions:
Now, we compare the given temperature and pressure with the critical temperature and pressure of CO2:
Temperature (T) < Critical Temperature (Tc): 305.15 K < 30.98°C Since the given temperature is higher than the critical temperature, CO2(g) will not be in the supercritical state at 32°C.
Pressure (P) > Critical Pressure (Pc): 80 atm > 73 atm The given pressure is higher than the critical pressure, indicating that the pressure is sufficient to liquefy CO2.
Based on these comparisons, CO2(g) can indeed be liquefied at 32°C and 80 atm pressure, as the pressure exceeds the critical pressure required for liquefaction. However, it's important to note that the temperature is above the critical temperature, so the CO2 will not be in a supercritical state. Instead, it will be in a gaseous state at this temperature and pressure.
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