Evaporation is one of the main methods used in chemical industry for concentration of aqueous solutions that means the removal of water from solution by boiling the liquor in a suitable type of evaporator and withdrawing the vapor (Coulson & Richardson‚1983). The objective of evaporation is to concentrate a solution consisting of non-volatile solute and a volatile solvent. In the overwhelming majority of evaporations the solvent is water. Normally‚ in evaporation the thick liquor is the valuable
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Experiment 2: Intermolecular Forces Performed: 9/12/2011 Submitted: 9/20/2011 Chemistry 1046L PART I: Purpose: The purpose of partI in this experiment is to identify a variety of unknown substances’ properties using observations of the temperature changes that occur during evaporation. We know that substances with weaker intermolecular forces‚ such as London dispersion‚ will have a faster vaporization rate and thus a higher temperature difference compared to
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Van der Waal’s forces -- Electrons will not be evenly spread around an atom/molecule at any given time‚ meaning the molecule will have a slight +ve charge on one end‚ and a -ve at the other. this temporary state may cause attraction between two molecules‚ pulling them together (also known as London dispersion forces). The magnitude pof Van der Waals force depends on the relative molecular mass‚ high mass produces a larger force. Boiling points of the alkanes data and alkenes data These very
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Intermolecular Bonding Essay Write an essay on intermolecular bonding. Explain how each type of bond arises and the evidence for the existence of each. Comment on their strengths in relation to the types of atoms involved; the covalent bond and relative to each other. Use the concepts of different types and strengths of intermolecular bonds to explain the following: There exists four types of intermolecular bonding‚ they include ionic‚ covalent‚ Van der waals and hydrogen bonding. In order to
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Internal Assessment: Rate of Evaporation Ann George Mr. Frias/4th Period Wheeler High School Research Question How will changing the molar mass of alcohol affect the rate of evaporation‚ represented by the change in temperature over time‚ measured using a temperature probe? Research/Abstract Alcohol is an organic compound in which the hydroxyl functional group‚ OH‚ is bound to a carbon atom. Its carbon center should be saturated; it should have single bonds to three other atoms. The different types
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Chemistry Project on Evaporation of Liquid Acknowledgement I would like to show my gratitude to my Chemistry Teachers Ms Seema More without whose support and encouragement this project could never have have taken the present shape . I would also like to thank my lab incharge Mr. Kakde For helping Me out During The Practical Part Of This Project. Aim Acknowledgment I am are greatly thankful for the cooperation and help from the Community Science Center (CSC) authorities and the Chemistry lab
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An experiment to find the percentage of three separated components Research Question: Is it possible to separate salt‚ sand and iron filings from each other in a mixture‚ to figure out the percentage of each component in the original mixture? Background Research: In this Investigation‚ I will be separating sand‚ salt‚ iron fillings in a mixture and finding their percentages. Iron is a magnetic solid which is incapable of being dissolved in water. Salt is a non-magnetic solid which is capable
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A. Comparison of Volatility by Rate of Evaporation Volatility describes how easily a substance will vaporize (turn into a gas or vapor). A volatile substance can be defined as (1) a substance that evaporates readily at normal temperatures and/or (2) one that has a measurable vapor pressure. The vapor pressure of a substance is the pressure at which its gaseous (vapor) phase is in equilibrium with its liquid or solid phase. It is a measure of the tendency of molecules and atoms to escape from a liquid
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Have you ever seen dry ice‚ well let me show you. To measure the evaporation rate it is important to know that a half pound of dry ice will be placed outside and timed. The same thing will happen but in a cool room. If the dry ice is -109.3°F then it will evaporate in any condition warmer. The hypotheses is that the dry ice in the outside will evaporation faster. It is important to understand this because if you are trying to store dry ice and you put it in a freezer it will still evaporate. So in
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With the measuring cups it was difficult to tell whether or not the estimation was correct. If the experiment were to be done again‚ it would have ice in the measuring cups to see how the cold would make any changes in the evaporation. The experiment was done because evaporation is something that is interesting to see what happens after the experiment is over. The experiment was done by making the water have different additives in it and seeing which one evaporates first. The results in the first
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