Characteristics Of Gases

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Jan Parker

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What Do You Think of When you Hear The Word “Gas”

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Factors Affecting Solubility and Rate of Dissolution Solubility is the ability of a substance to be dissolved in another substance at a specific temperature and pressure. It is also defined as the maximum amount of solute that can be dissolved in a given amount of solvent at a specified temperature and pressure to produce a solution in equilibrium. It is usually expressed in grams of solute per milliliters of solvent. Factors Affecting Solubility 1. Nature of Solute and Solvent A solute can only be dissolved in a solvent when they are “alike.” A general rule is “like dissolves like.” 2. Temperature The solubility of a solid and liquid solute increases when temperature is increased. The solubility of a gaseous solute to a liquid solvent decreases as temperature increases. 3. Pressure The effect of pressure is only applicable for the solubility of gases in liquids. The higher the pressure of a gas, the more soluble it is. Rate of Dissolution The rate of dissolution is defined as how fast a solute dissolves in a given solvent at a specific temperature. The process of dissolving a solute is called dissolution. Factors Affecting the Rate of Dissolution 1. Stirring Stirring a solute will increase its rate of dissolution. When you stir, solute particles come into closer contact more often with solvent particles. 2. Size of the solute particle The smaller the particles of the solute, the faster it dissolves in the solvent. Small particles provide larger surface area for contact with the solvent. 3. Temperature As temperature increases, the rate of dissolution of solid and liquid solutes also increases. 4. Amount of solute present in a solution When you have little amount of solute in the solution, it is easier to dissolve the same solute in the given solvent. However, when you have a lot of solute already present in the solvent, dissolution takes slowly.

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Physical laws related to gases Gases diffuse from an area of Higher concentration gradient to an area of lower concentration gradient. The pressure with which a gas tends to come out of the gas mixture is called partial pressure. Total partial pressure of a gas mixture is the sum of partial pressures of the gases in the mixture e.g. atmospheric pressure is the sum of partial pressure of gases in atmosphere. Pressure is caused by multiple impacts of moving molecules against a surface. Partial pressure of a gas is directly proportional to the concentration of the gas molecules Concentration of dissolved gas = Pressure X solubility coefficient Or Partial Pressure of a gas = Concentration of dissolved gas/ solubility coefficient Concentration of dissolved gas = Pressure X solubility coefficient Or Partial Pressure of a gas = Concentration of dissolved gas/ solubility coefficient If the partial pressure is greater in the gas phase in the alveoli, as is normally true for oxygen, then more molecules will diffuse into the blood than in the other direction. If the partial pressure of the gas is greater in the dissolved state in the blood, which is normally true for carbon dioxide, then net diffusion will occur toward the gas phase in the alveoli At normal body temperature of 37°C the vapor pressure is 47 mm of Hg. The vapor pressure of water depends entirely on the temperature of the water. The greater the temperature, the greater the kinetic activity of the molecules and, therefore, the greater the likelihood that the water molecules will escape from the surface of the water into the gas phaseIt is defined as: “ It is a constant, which is the measure of a substance diffusing through the concentration gradient.”

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