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- Vapour pressure, also known as vapour equilibrium pressure, can be defined as the pressure exerted (in a system featuring thermodynamic equilibrium) by a vapour with its condensed phases (solid or liquid) in a closed system at a given temperature.
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Vapour pressure, also known as vapour equilibrium pressure, can be defined as the pressure exerted (in a system featuring thermodynamic equilibrium) by a vapour with its condensed phases (solid or liquid) in a closed system at a given temperature.
- 2 min
- A liquid’s vapour pressure is a vapour’s equilibrium pressure above its liquid (or solid); that is, the vapour pressure resulting from a liquid (or...
- Raoult’s law is a chemical law that relates the solution’s vapour pressure to the mole fraction of a solution added. The law of Raoult is expressed...
- When a liquid’s vapour pressure is the same as the atmospheric pressure, the material is at temperature and pressure at the boiling/freezing point....
- As a result, there are lower boiling points of liquids with high vapour pressure. By heating a liquid and allowing more molecules to enter the atmo...
- The material with the lowest boiling point would, therefore, have the highest vapour pressure at room temperature (the easiest way to reach the gas...
- UNIT 7
- 7.1 EQUILIBRIUM IN PHYSICAL PROCESSES
- 7.1.2 Liquid-Vapour Equilibrium
- 7.1.4 Equilibrium Involving Dissolution of Solid or Gases in Liquids Solids in liquids
- Gases in liquids
- 7.1.5 General Characteristics of Equilibria Involving Physical Processes
- 7.2 EQUILIBRIUM IN CHEMICAL PROCESSES – DYNAMIC EQUILIBRIUM
- 7.6 APPLICATIONS OF EQUILIBRIUM CONSTANTS
- 7.8 FACTORS AFFECTING EQUILIBRIA
- 7.8.3 Effect of Inert Gas Addition
- 7.8.5 Effect of a Catalyst
- 7.9 IONIC EQUILIBRIUM IN SOLUTION
- Solution
- 7.11.7 Factors Affecting Acid Strength
- 7.12.1 Designing Buffer Solution
- 7.13 SOLUBILITY EQUILIBRIA OF SPARINGLY SOLUBLE SALTS
- 7.13.2 Common Ion Effect on Solubility of Ionic Salts
- SUMMARY
- SUGGESTED ACTIVITIES FOR STUDENTS REGARDING THIS UNIT
After studying this unit you will be able to identify dynamic nature of equilibrium involved in physical and chemical processes; state the law of equilibrium; explain characteristics of equilibria involved in physical and chemical processes; write expressions for equilibrium constants; establish a relationship between Kp and Kc; explain various fac...
The characteristics of system at equilibrium are better understood if we examine some physical processes. The most familiar examples are phase transformation processes, e.g., solid liquid liquid gas solid gas
This equilibrium can be better understood if we consider the example of a transparent box carrying a U-tube with mercury (manometer). Drying agent like anhydrous calcium chloride (or phosphorus penta-oxide) is placed for a few hours in the box. After removing the drying agent by tilting the box on one side, a watch glass (or petri dish) containing ...
We know from our experience that we can dissolve only a limited amount of salt or sugar in a given amount of water at room temperature. If we make a thick sugar syrup solution by dissolving sugar at a higher temperature, sugar crystals separate out if we cool the syrup to the room temperature. We call it a saturated solution when no more of solute ...
When a soda water bottle is opened, some of the carbon dioxide gas dissolved in it fizzes out rapidly. The phenomenon arises due to difference in solubility of carbon dioxide at different pressures. There is equilibrium between the molecules in the gaseous state and the molecules dissolved in the liquid under pressure i.e., CO (gas)
For the physical processes discussed above, following characteristics are common to the system at equilibrium: Equilibrium is possible only in a closed system at a given temperature. Both the opposing processes occur at the same rate and there is a dynamic but stable condition. All measurable properties of the system remain constant. When equilibri...
Analogous to the physical systems chemical reactions also attain a state of equilibrium. These reactions can occur both in forward and backward directions. When the rates of the forward and reverse reactions become equal, the concentrations of the reactants and the products remain constant. This is the stage of chemical equilibrium. This equilibriu...
Before considering the applications of equilibrium constants, let us summarise the important features of equilibrium constants as follows: Expression for equilibrium constant is applicable only when concentrations of the reactants and products have attained constant value at equilibrium state. The value of equilibrium constant is independent of ini...
One of the principal goals of chemical synthesis is to maximise the conversion of the reactants to products while minimizing the expenditure of energy. This implies maximum yield of products at mild temperature and pressure conditions. If it does not happen, then the experimental conditions need to be adjusted. For example, in the Haber process for...
If the volume is kept constant and an inert gas such as argon is added which does not take part in the reaction, the equilibrium remains undisturbed. It is because the addition of an inert gas at constant volume does not change the partial pressures or the molar concentrations of the substance involved in the reaction. The reaction quotient changes...
A catalyst increases the rate of the chemical reaction by making available a new low energy pathway for the conversion of reactants to products. It increases the rate of forward and reverse reactions that pass through the same transition state and does not affect equilibrium. Catalyst lowers the activation energy for the forward and reverse reactio...
Under the effect of change of concentration on the direction of equilibrium, you have incidently come across with the following equilibrium which involves ions: Fe3+(aq) + SCN–(aq) [Fe(SCN)]2+(aq) There are numerous equilibria that involve ions only. In the following sections we will study the equilibria involving ions. It is well known that the aq...
Hydroxyl ion is a Lewis base as it can donate an electron lone pair (:OH–). Flouride ion acts as a Lewis base as it can donate any one of its four electron lone pairs. A proton is a Lewis acid as it can accept a lone pair of electrons from bases like hydroxyl ion and fluoride ion. BCl acts as a Lewis acid as it can 3 accept a lone pair of electrons...
Having discussed quantitatively the strengths of acids and bases, we come to a stage where we can calculate the pH of a given acid solution. But, the curiosity rises about why should some acids be stronger than others? What factors are responsible for making them stronger? The answer lies in its being a complex phenomenon. But, broadly speaking we ...
Knowledge of pK a, pK and equilibrium b constant help us to prepare the buffer solution of known pH. Let us see how we can do this.
We have already known that the solubility of ionic solids in water varies a great deal. Some of these (like calcium chloride) are so soluble that they are hygroscopic in nature and even absorb water vapour from atmosphere. Others (such as lithium fluoride) have so little solubility that they are commonly termed as insoluble. The solubility depends ...
It is expected from Le Chatelier’s principle that if we increase the concentration of any one of the ions, it should combine with the ion of its opposite charge and some of the salt will be precipitated till once again K = sp Q sp. Similarly, if the concentration of one of the ions is decreased, more salt will dissolve to increase the concentration...
When the number of molecules leaving the liquid to vapour equals the number of molecules returning to the liquid from vapour, equilibrium is said to be attained and is dynamic in nature. Equilibrium can be established for both physical and chemical processes and at this stage rate of forward and reverse reactions are equal. Equilibrium constant, K ...
The student may use pH paper in determining the pH of fresh juices of various vegetables and fruits, soft drinks, body fluids and also that of water samples available. The pH paper may also be used to determine the pH of different salt solutions and from that he/she may determine if these are formed from strong/weak acids and bases. They may prepar...
If a non-volatile solute is added to a solvent to give a solution [Fig. 2.4.(b)], the vapour pressure of the solution is solely from the solvent alone. This vapour pressure of the solution at a given temperature is found to be lower than the vapour pressure of the pure solvent at the same temperature.
Vapour pressure can be defined as pressure formed by the vapor of the liquid (or solid) over the surface of the liquid. This pressure is formed in a thermodynamic equilibrium state in a closed container at a certain temperature. Liquid’s evaporation rate is identified by the equilibrium vapor pressure.
6 days ago · Vapour pressure can be defined as a measurement of a material's tendency to change state from solid to liquid to gas or vapour when the temperature rises. It represents the rate at which a liquid evaporates. It's also linked to the tendency for particles to escape from a liquid or solid state.
Nov 4, 2023 · Chapter 1: Chemical Reactions and Equations. NCERT Solutions for class 10 Science. Chapter 2: Acids, Bases and Salts. Chapter 3: Metals and Non-Metals. Chapter 4: Carbon and its Compounds. Chapter 5: Periodic Classification of Elements. Chapter 6: Life Processes. Chapter 7: Control and Coordination. Chapter 8: How do Organisms Reproduce?
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