Charles Law Formula Charles Law Formula harles's law (also known as the law of volumes) is an experimental gas law which describes how gases tend to expand when heated. A modern statement of Charles' law is: At constant pressure, the volume of a given mass of an ideal gas increases or decreases by the same factor as its temperature on the absolute temperature scale (i.e. the gas expands as the temperature increases). Charles Law :- Jacques Charles Law describes the relationship between volume and temperature of gases. This law is named after Jacques Charles who studied the relationship between volume (V) and temperature (T) around the turn of the 19th century. He determined this law for the equal amount of gases at constant pressure. VT = constant This defines a direct relationship which means 'an increase in one results in an increase in the other'
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Note :- "At constant pressure, the volume of a given mass of gas increases or decreases by 1/273 of its original volume at 32oF, for each degree centigrade rise or lowering in temperature." Charles Law Definition :- Charles law states that at constant pressure the volume of the gas is directly proportional to the temperature of the gas. The Law can be understood by keeping the pressure constant. When the temperature of the gas is increased the volume of the gas increases. Charles law gives a direct relationship between the volume of the gas and the temperature of the gas. Simple problem on conversion of temperature scale from °C to K 1. Convert 35°C to Kelvin Solution Formula for the conversion from °C to Kelvin is Temperature in K = °C + 273.15 So 35°C + 273.15 = 308.15 K 2. Convert 298.15K to °C Solution Formula for the conversion from Kelvin to °C is Temperature in °C + 273.15 = K °C = temperature in K -273.15 So 298.15 - 273 = 25°C Charles Law explanation
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The explanation of the Charles law can be given by the fact that the average molecular motion, i.e., the speed of the gases depends on the temperature. With increase in the temperature, average velocity of the gas molecules increases and they can move around the container with greater speed. When the temperature is increased to keep the pressure constant, i.e., the number of collisions with the walls of the container, the volume of the gas is increased. So the temperature and volume are closely related and a particular temperature is needed by the gas molecules to keep its random motion. If the temperature is not enough to keep the random motion, the molecules tends to move slowly and they are attracted to each other by weak vander walls forces of attraction and hence they become liquid or solid.
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