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The grignard reaction lab report tamu chem
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Ishaan Sangwan Experiment 7: Grignard Reaction Discussion In this experiment, a Grignard reaction was performed to create a carbon-carbon bond, between a bromide and carbon dioxide. The product was then protonated to form a carboxylic acid, which was identified by obtaining its melting point, and by performing a titration with NaOH to obtain its molecular weight. In organometallic chemistry, carbon is bound to a metal. Usually, carbons are bound to elements that are more electronegative than carbon, and have a partial positive charge, making them electrophilic. When a carbon is bound to a metal, it has a partial negative charge, since it is more electronegative than the metal, and is hence nucleophilic. A nucleophilic carbon can then attack …show more content…
Had these pockets not been filled, they could have been filled by diethylether vapor, which would have frozen these joints. The Mg used in this experiment was crushed, and then reacted with iodide in order to bring fresh Mg to the surface to improve the reaction. The formation of MgI2 was also exothermic, which added heat to help start the reaction. A liquid solid extraction was performed in this experiment to remove impurities that had sank to the bottom on the flask, like unreacted bromide and the aforementioned side products. Then, a liquid liquid extraction was performed to pull the carboxylic acid into an aqueous sodium hydroxide layer from the organic ether layer. The molecular weight of the unknown was calculated by figuring out how many moles of NaOH reacted with the unknown. Since there ratio of reactants reacting was 1:1, the moles of NaOH would be the same as the moles of carboxylic acid. The moles of NaOH were calculated by multiplying the concentration of NaOH by the volume used in the titration. The molecular weight of he carboxylic acid was then calculated by dividing the mass of the carboxylic acid sample by the number of moles of carboxylic
Greta Christina eloquently puts into words something I know in theory, but can be hard to understand in practice in heterosexual relationships. In Are we having sex now or what? Christina details her record keeping of how many people she had sex with, and what she counted as sex. She talks about the limiting misconception of sex only being coitus, and other acts not “counting.” Christina writes of how when she started having sex with women her outdated system of what was sex and what was not sex was completely destroyed. By limiting sex to “penis in vagina,” Christina was discounting some of her favorite sexual experiances, and including ones she did not particularly enjoy.
In the second reaction, 3.25 grams of NaOH was used, or 3.25/(23.0+16.0+1.0) = 0.08125 mol of NaOH. 200/1000 = 0.2 liter of 0.25 M HCl was used, or 0.25(0.2) = 0.05 mol of HCl. As the reaction occurred in a one-to-one ratio (1 mol of NaOH per 1 mol of HCl), there were far more NaOH available than what can be reacted with
Thermochemistry is the study of energy changes that occur during chemical reactions and changes in state. There are two different processes that have to do with the absorption and release of heat. In the endothermic process, the system picks up heat, as the surroundings lose heat. In the exothermic process, heat is released to its surroundings. Heat either goes in or goes out.
This report discusses several different types of chemical reactions that were conducted in a lab. A chemical reaction is when two or more chemicals interact to form a new substance or rearrange the molecules within the substances. There are many signs that indicate when a chemical reaction has occurred. These changes include: a colour change, a gas being formed, a solid being formed, a change in temperature, precipitates are formed, a change in smell, light being emitted, a change in mass or volume, a change in conductivity, a change in boiling and/or melting point, and a change in taste. In the lab, thirteen different chemical reaction were conducted. Five of these reactions were single displacement reactions. A single displacement reaction is a reaction in which an element
An endothermic reaction is a chemical reaction that absorbs heat into its environment. The energy is usually transferred as heat energy, causing its surroundings to get colder. The opposite to an endothermic reaction is an exothermic reaction. An exothermic reaction releases cold energy which absorbs heat energy. As a result of this, the surroundings distinctively become hotter. In this experiment an exothermic reaction takes place.
Divide the mass of unknown A by its respective amount of moles to find its molar mass. Record the data. Repeat steps 3-6 for unknowns B, C and D. Compare the unknowns’ molar masses to each known compound’s molar mass in order to determine its identity. DATA AND OBSERVATIONS Known Compounds Compound Molar Mass
Then CsCO3 and bromooctadecane was added to the solution. And at the end we crystalized it and found out the melting point which ranged from 64-68°C. Theory: In order for an ether to be produced we needed an aroxide ion and an alkyl halide.
To determine if the mass increases when we burn the magnesium and change it into magnesium oxide
The question posed for the conservation lab was: what happens to the mass of a system in a chemical reaction? When new substances are produced in a reaction we say a chemical change has occurred. These changes are very difficult, sometimes impossible, to reverse. Atoms are not created or destroyed in a chemical reaction, they are just rearranged from the reactants to form the products. This is the reason why symbol equations must be balanced. If a chemical reaction is completed in a closed system (when nothing extra can get in and nothing can escape), then the mass will remain constant. But, if the chemical reaction happens in an open system (where air can get in and out), then mass may appear to change.
The exothermic reaction observed in this procedure is as follows ; HCL(aq) + NaOH(aq) ➡ H2O(l) + NaCL(aq) + energy. The purpose of the lab was to determine the value of ∆H of the neutralization reaction above, then compare the data to that of the accepted ∆H value of neutralization to determine the accuracy and validity of our findings. A singular trend was observed and is as follows; the decrease of ∆H indicates a reaction is exothermic, a neutralization reaction results in a (-) value ∴ the (-) value collected was congruent with the trend above, proving our results have some legitimacy at the least.
We write the mole ratio (conversion factor with dimensional analysis): (Unknown subtance)/(Known substance)=(1 mol N_2)/(2 mol 〖NH〗_3 ) Step 3: Multiplication We multiply the known substance (number of moles) by the conversion factor (mole ratio) to obtain the unknown substance (number of
In the titration experiment, the endpoint was recorded in the experimental data to be at 21.30 mL of NaOH and at a pH of 10.44. However, when all of the data from the table was graphed, the observed endpoint was too high up and on a part of the upper concave down portion of the graph. To ensure that the proper equivalence point was used, a new point had to be extrapolated that was roughly the point at which the graph went from concave up to concave down. This point was at 21.28 mL of NaOH added and pH of 9.20. Dividing both of these points by two, the half equivalence point was found to be at a pH of 5.30 and 10.64 mL of NaOH added. The pH is equal to the pKa here, so the pKa was found to be 5.30. Using data from the equivalence point extrapolated from the graph, the molar mass of the unknown was calculated to by 148 grams per mole. Lastly, because there was only one region of
As you across a period, of metals, the reactivity decreases. The reactivity decreases because the atomic radius decreases as well. As the atomic radius increases, ionization energy and electronegativity increase, because the effect of shielding isn't as great as it is on smaller atoms. A larger ionization energy means that the atom is less prone to giving electrons and a larger electronegativity means that the atom has more of an attraction on other atoms'
My most recent team experience was in Chemistry II class. We performed a group lab experiment, where we were given two unknown substances and had to figure out what they were by using different chemical reactions. With this lab, my team and I had to work together to observe the chemical reactions that the substances were making, so we could compare them to our unknown substances. My team and I observed all of these reactions together and helped each other with the color observations because one of our team members is partially color blind. In the end with all of our observations our conclusion for the two unknown substances was correct. Working with this team was an extraordinary example of what being a good teammate is all about. Good teammates
The initial and final volumes of NaOH were compared after the solution was titrated in five different