Understanding How Chemists View Molecules: The Laws of Definite and Multiple Proportions
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1 Understanding How Chemists View Molecules: The Laws of Definite and Multiple Proportions Name: Period: The period from was critical for the development of chemistry. During that time period, quantitative data was first collected on the synthesis of many different kinds of compounds. Studying this data allowed several individuals, namely Antoine Lavoisier, Joseph Proust, and John Dalton to elucidate the three primary laws of chemical composition. The first of these laws, the Law of Conservation of Mass, states that in any chemical process, mass is neither created nor destroyed. Using this law as a basis, it was obvious that chemical compounds obeyed certain mathematical relationships, namely the Laws of Definite and Multiple Proportions. Using these laws, John Dalton, an English schoolteacher, was able to develop the atomic theory, which is our basis for beginning to understand how substances combine on an atomic level. The goal is this experiment is to mimic simple synthesis experiments performed by chemists over 200 years ago. The data generated in this lab should clarify both what the Laws of Definite and Multiple Proportions are, and how you use them. MATERIALS: Each Group of 4 should have A cup with top Some Bolts Some Nuts A Balance PROCEDURE: 1) Label your cup and lid with a number. 2) Determine the mass of your cup and lid together 3) Select some bolts from your set (the number can range from 5 20). It doesn t matter how many bolts you choose. Record the number of bolts in the data table below. 4) Put the bolts in the cup and seal the cup with the lid. 5) Collaborate with 5 other groups (who have also put their bolts in their cup). Using the balance, determine the mass of the other group s sealed cup with bolts. In addition, the other groups will give you the mass of their empty cup. Record both the number of the cup and the mass of the cup, and cup with bolts in the table below. My Cup #: Mass of Empty Cup: Number of Bolts in Cup:
2 Table I: Cup and Bolt Data Cup Number Mass of Empty Cup Mass of Cup + Bolts 6) Now create a model of the compound BN x by attaching a fixed number of nuts to each bolt. For example, if you wanted to a sample of BN 2, you would screw on two bolts to each nut. Do this for all of your bolts, and inform the instructor of the formula of your compound. Place the formula of your compound in the space below. Formula of Compound: 7) Make a molecule for each bolt in your cup and then place the molecules into the cup and seal it. Other groups will be doing the same thing. When everyone is done, rejoin the other groups you collaborated with, and determine the mass of each cup filled with sample. Place this value in the table below. Table II: Sample Product Data Cup Number Mass of Cup + product ANALYSIS (all calculations will go into Table III, below) 1) Determine the mass of the bolts in each cup by subtracting the mass of the cup from the mass of the cup and bolts. Perform one sample calculation, and place the rest of the results in Table III, below. SAMPLE CALCULATION:
3 2) Determine the mass of product in each cup, performing one sample calculation, and placing the results in Table III, below: SAMPLE CALCULATION: Complete the table below, using the law of conservation of mass to first determine the mass of nuts in each product. Then determine the ratio of the mass of nuts to the mass of bolts, showing a sample calculation of each type below. SAMPLE CALCUALTION: Table III: Examining the Ratios of Nuts and Bolts Cup Number Mass of Bolts (determined from Table I) Mass of Product (determined from Table II) Mass of nuts in Product Ratio of Mass of Nuts to Mass of Bolts Questions: 1) How many different compounds did you study? Explain 2) Does your data satisfy the law of definite proportions? Explain
4 2) Was it necessary to know how many bolts where in a cup to obtain this information? Explain 3) What is the relative mass of one nut to one bolt? Justify your answer 4) Given that fact that you know the formula of your compound, determine the formula of the other compounds in the table above. Place your answers for each cup in the table below. Justify your reasoning Table IV: The Formula of the Compound in Each Cup Cup Number Formula
5 5) State the law of multiple proportions. Based on our discussion in class, show that the data satisfy this law. QUESTIONS: 1) As we have discussed in class, Dalton used definite and multiple proportions to support his atomic theory. State the postulates of the atomic theory: 1) 2) 3) 4) How does atomic theory explain (use your data as an example): a) The fact that the ratio of the masses of elements in a compound is always fixed?
6 b) The law of multiple proportions? 2) If someone defined the relative mass of a bolt to be 100. g, what would be the relative mass of a nut? 3) Consider glucose, C 6 H 12 O 6. A biology student finds a sample of glucose that contains 45 g of carbon. a) How many grams of oxygen are in the compound? b) What is the total mass of the glucose sample? c) Can you determine the number of molecules of glucose in the sample? Explain CONCLUSION:
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