'Stoichiometry Lab\r'

'Stoichiometry February 28th, 2013 Abstract: The fight downions of the sodium hydroxide and deuce acids, Hydrochloric Acid and Sulfuric Acid were performed. The horniness given off by these two responses was apply to determine the stoichiometric ratio and the limiting reactants in each experiment. Introduction: Coefficients in a equilibrize equations show how many moles of each reactant is needed to react with each other and how many moles of each intersection that will be formed. Stoichiometry allows us to calculate the summation of reactants needed and excessively the inwardness of product.The major innovation of stoichiometry is formed by the law of definite ratios, which states that a chemical compound always contains the exact proportion of elements by mass. This is withal the heart of balancing chemical equations. The coefficients of a balanced equation send packing also be thought of as the ratios in which the reactants combine. In the chemical equation A+ B> AB t he coefficients secure us that for every one mole of reactant â€Å"A” one moles of reactant â€Å"B” ar needed and use to produce the product â€Å"AB”.If two moles of â€Å"A” was present and further one mole of â€Å"B” the excess mole of â€Å"A” would have zilch to react with. In this reaction â€Å"B” would be the limiting reactant. The reaction is limited due to â€Å"B” because once â€Å"B” is all used up, the reaction will stop, and there would be an excess of unused â€Å"A”. The progress of a reaction can be mensural by the pepperiness heartiness that is given off. Exothermic reactions give off rut and therefore an increase in temperature also occurs. The reaction between an acid and a base is also known as neutralization, and is usually an exothermic reaction.When reactants are combined at stoichiometric ratios the reaction is fitting to be completed and would exert the most heat energy. Th e purpose of this lab was to carry out the reaction between a basic solution of Sodium hydroxide with Hydrochloric acid, and also the reaction of Sodium Hydroxide with Sulfuric Acid to determine the limiting reactant and the stoichiometric ratio of each experiment. Procedure: Reaction in the midst of HCL and NaOH Diluted Solutions of HCL and NaOH were prepared. cxx ml of 3M stock of HCl and NaOH were thrifty with a gradatory cylinder and placed into two 250 ml beakers.Two 400ml beakers were filled with 240 ml of peeing measured by graduated cylinder. The 120ml of HCl was added to one of the beakers containing water and the 120 NaOH to the other, both being added slowly while aspiration the solution vigourously. Label the beakers HCl and NaOH. Keep the beakers covered with a watch glass when not in use. verse and record the temperature of the NaOH solution apply the PASCO Explorer temperature try. obtain sure to rinse off and dry the probe after every use. Obtain a coffee cup calorimeter and chapeau to house the reactions.Measure the appropriate amount HCl (see graph A) pour it in the calorimeter and determine its temperature using the temperature probe. get in the temperature. Measure the corresponding amount of NaOH (see map A) and add it to the calorimeter all at once. Put the lid back on the calorimeter and stir it carefully with the probe. Record the highest temperature reached as the reaction occurs. Rinse the cup with deionized water and dry. Repeat experiment for each of the amounts of chart A. chart A) Amount of each reactant l 1. 0 M Acid| 55. 0| 50. 0| 45. 0| 40. 0| 35. 0| 30. 0| 25. 0| 20. 0| 15. 0| 10. 0| 5. 0| ml 1. 0 M NaOH| 5. 0| 10. 0| 15. 0| 20. 0| 25. 0| 30. 0| 35. 0| 40. 0| 45. 0| 50. 0| 55. 0| *Use 100 ml graduated cylinder for measuring volumes 30 to 55 ml, 25 ml graduated cylinder for volumes 15ml through 25 ml, and 10 ml graduated cylinder for volumes 5ml and 10 ml Reaction Between H? SO? and NaOH Use the procedure from the Reaction Between HCL and NaOH only substitute the HCl with H? SO? , and the same amounts listed in chart A.\r\n'