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Standard X

Physics

Phase Change

Mark the corr...

Question

Mark the correct statement(s) based on the phase diagram of $C O_{2}$ shown in the graph.

298K is the normal boiling point of liquid

C O_{2}

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At 1 atm & 190 K

C O_{2}

will exist as gas.

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C O_{2} (s)

will sublime above 195K under normal atmospheric pressure.

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Melting point & boiling point of

C O_{2}

will increase on increasing pressure.

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Solution

The correct options are
C $C O_{2} (s)$ will sublime above 195K under normal atmospheric pressure.
D Melting point & boiling point of $C O_{2}$ will increase on increasing pressure.
When pressure is 1 atm and temperature is slightly lower than 195K, carbon dioxide exist in solid state. When pressure is kept constant and temperature is increased, phase transformation from solid to gas occurs. At this point, there is no liquid phase. Hence, solid carbon dioxide will sublime above 195K under normal atmospheric pressure.

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Similar questions

Q. Answer the following questions based on the P-T phase diagram of carbon dioxide: (a) At what temperature and pressure can the solid, liquid and vapour phases of CO2 co-exist in equilibrium ? (b) What is the effect of decrease of pressure on the fusion and boiling point of CO2 ? (c) What are the critical temperature and pressure for CO2 ? What is their significance ? (d) Is CO2 solid, liquid or gas at (a) –70 °C under 1 atm, (b) –60 °C under 10 atm, (c) 15 °C under 56 atm ?

Q. Answer the following questions based on the P-T phase diagram of carbon dioxide:

(a) At what temperature and pressure can the solid, liquid and vapour phases of

C O_{2}

co-exits in equilibrium ?

(b) What is the effect of decrease of pressure on the fusion and boiling point of

C O_{2}

C O_{2}

? what is their significance ?

(d) Is

C O_{2}

solid, liquid or gas at (a)

- 70^{o} C

under 1 atm, (b)

- 60^{o} C

under 10 atm, (c)

15^{o} C

under 56 atm ?

Isotherms of carbon dioxide at various temperatures are represented in figure. Answer the following based on this figure.

(i) In which state will $C O_{2}$ exist between the points a and b at temperature $T_{1}$ ?

(ii) At what point will $C O_{2}$ start liquefying when temperature is $T_{1}$ ?

(iii) At what point will $C O_{2}$ be completely liquefied when temperature is (T_2\)

(iv) Will condensation take place when the temperature is $T_{3}$ ?

(v) What portion of the isotherm at $T_{1}$ represent liquid and gaseous $C O_{2}$ at equilibrium?

Q. What will be the effect of increased concentration of

C O_{2}

in blood on normal breathing?

Q. Henry's law constant for

{C O}_{2}

in water is

1.67 \times 10^{8}

Pa at 298K. Calculate the quantity of

{C O}_{2}

in 500 ml of soda water when packed under 2.5 atm

{C O}_{2}

pressure at 298 K.

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Mark the correct statement(s) based on the phase diagram of CO2 shown in the graph.

Mark the correct statement(s) based on the phase diagram of $C O_{2}$ shown in the graph.