Home
Class 11
PHYSICS
Assertion At triple point, three stated ...

Assertion At triple point, three stated (solid, liquid and gas) may co-exist simulaneously.
Reason For water, the values of pressur and temperature corresponding to triple point are 10 mm of Hg and 273.16 K.

A

If both Assertion and Reason are correct and Reason is the correct explanation of Assertion.

B

If both Assertion and Reason are correct but Reason is not the correct explation os Assertion.

C

If Assertionis true bur Reason is false.

D

If Assertion is false but Reason is true.

Text Solution

AI Generated Solution

The correct Answer is:
To solve the question, we need to analyze the assertion and the reason provided. ### Step 1: Understand the Assertion The assertion states that "At the triple point, three states (solid, liquid, and gas) may coexist simultaneously." - **Explanation**: The triple point of a substance is defined as the specific temperature and pressure at which all three phases (solid, liquid, and gas) can exist in thermodynamic equilibrium. This means that at the triple point, ice (solid), water (liquid), and water vapor (gas) can all be present at the same time. ### Step 2: Evaluate the Reason The reason states that "For water, the values of pressure and temperature corresponding to the triple point are 10 mm of Hg and 273.16 K." - **Explanation**: The correct values for the triple point of water are approximately 4.58 mm of Hg for pressure and 273.16 K for temperature. The reason provided in the question incorrectly states the pressure as 10 mm of Hg, which is not accurate. ### Step 3: Conclusion - The assertion is **true** because at the triple point, all three phases can coexist. - The reason is **false** because the pressure value given (10 mm of Hg) is incorrect. ### Final Answer Thus, the correct conclusion is that the assertion is true, but the reason is false.
To solve the question, we need to analyze the assertion and the reason provided. ### Step 1: Understand the Assertion The assertion states that "At the triple point, three states (solid, liquid, and gas) may coexist simultaneously." - **Explanation**: The triple point of a substance is defined as the specific temperature and pressure at which all three phases (solid, liquid, and gas) can exist in thermodynamic equilibrium. This means that at the triple point, ice (solid), water (liquid), and water vapor (gas) can all be present at the same time. ### Step 2: Evaluate the Reason ...
Promotional Banner

Topper's Solved these Questions

  • THERMOMETRY THERMAL EXPANSION AND KINETIC THEORY OF GASES

    DC PANDEY ENGLISH|Exercise Match the columns|5 Videos

  • THERMOMETRY THERMAL EXPANSION AND KINETIC THEORY OF GASES

    DC PANDEY ENGLISH|Exercise Medical entrance gallary|30 Videos

  • THERMOMETRY THERMAL EXPANSION AND KINETIC THEORY OF GASES

    DC PANDEY ENGLISH|Exercise A Tacking it together|55 Videos

  • SUPERPOSITION OF WAVES

    DC PANDEY ENGLISH|Exercise Level 2 Subjective|8 Videos

  • THERMOMETRY,THERMAL EXPANSION & KINETIC THEORY OF GASES

    DC PANDEY ENGLISH|Exercise Level 2 Subjective|9 Videos

Similar Questions

Explore conceptually related problems

The point where all the three state (solid, liquid, vapour) of H_2O exist is known as

Define triple point of a substance. Write its value of temperature and pressure for water.

A closed flask contains a substance in all its three states, solids, liquids and vapour at its triple point. In this situation the average KE of the water molecule will be

Answer the following questions based on the p-T phase diagram of carbon dioxide as shown in the figure . (i) At what temperature and pressure can the solid , liquid and vapour phases of C0_(2) co-exist in equilibrium? (ii) What is the effect of decrease of pressure on the fusion and boiling point of C0_(2) ? (iii) What are the critical temperature and pressure for C0_(2) ? what is their significance ? (iv) Is C0_(2) solid , liquid, or gas at (a) -70^(@)C under 1 atm (b) -60^(@)C under 10 atm (c) 15^(@)C under 56 atm ?

Answer the following questions based on the p-T phase diagram of carbon dioxide as shown in the figure . (i) At what temperature and pressure can the solid , liquid and vapour phases of C0_(2) co-exist in equilibrium? (ii) What is the effect of decrease of pressure on the fusion and boiling point of C0_(2) ? (iii) What are the critical temperature and pressure for C0_(2) ? what is their significance ? (iv) Is C0_(2) solid , liquid, or gas at (a) -70^(@)C under 1 atm (b) -60^(@)C under 10 atm (c) 15^(@)C under 56 atm ?

Assertion:At low temperature , particles of matter occupy fixed positions and exist in solid state. Reason : Under a given set of conditions of temperature and pressure , the state of a substance depends upon the net effect of thermal energy and intermolecular forces.

Assertion : Bulk modulus of elasticity can be defined for all three states of matter, solid liquid and gas. Reason: Young's modulus is not defined for liquids and gases.

Each phase of a material can exits only in certain regions of pressure and temperature . P-T phase diagrams, in which pressure is plotted versus temperature, show the regions corresponding to various phases and phase transformations . P-V diagrams, on the other hand , can be used to study pressure volume relationship at a constant temperature. If the liquid and gaseous phases of a pure substances are heated together in a closed container, both the temperature and the vapor pressure will increase until a point is reached at which the two phases can no longer be distinguished from one another. The temperature and pressure at which this occurs are called the critical temperature and pressure. Exceeding either of these parameters, by itself ,will cause the "gas"//"liguid" phase transition to disappear. if the other variable is then changed as well, while the first variable is maintained above its critical point , a gradual transition will occur between the gaseous and liquid phases, with no clear boundary.(The liquid and solid phases, on the other hand , maintain a distinct boundary at all pressure above the triple point). Shown in figure is a combined P-T phase diagram for material A and B . If heat is added to solids A and B , each in a container that is open to the atmosphere :-

At room temperature, a dilute solution of urea is prepared by dissolving 0.60 g of urea in 360 g of water. If the vapour pressure of pure water at this temperature is 35 mm Hg, lowering of vapour pressure will be 1.74 xx 10^(-x) mm Hg. The numerical value of x is _____________. (Molar mass of urea = 60 g mol^(-1) ).

Each phase of a material can exits only in certain regions of pressure and temperature . P-T phase diagrams, in which pressure is plotted versus temperature, show the regions corresponding to various phases and phase transformations . P-V diagrams, on the other hand , can be used to study pressure volume relationship at a constant temperature. If the liquid and gaseous phases of a pure substances are heated together in a closed container, both the temperature and the vapor pressure will increase until a point is reached at which the two phases can no longer be distinguished from one another. The temperature and pressure at which this occurs are called the critical temperature and pressure. Exceeding either of these parameters, by itself ,will cause the "gas"//"liguid" phase transition to disappear. if the other variable is then changed as well, while the first variable is maintained above its critical point , a gradual transition will occur between the gaseous and liquid phases, with no clear boundary.(The liquid and solid phases, on the other hand , maintain a distinct boundary at all pressure above the triple point). Shown in figure is a combined P-T phase diagram for material A and B . Which is true about the substance in figure?