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1. Experimental Procedure, Part A.1. In the experiment, 2.00g of salicylic acid (molar mass =138.1g/mol ) reacts with an excess amount of acetic anhydride a. Calculate the theoretical yield of acetylsalicylic acid (molar mass =180.2g/mol ) for this synthesis. b. After completing the Experimental Procedure, a mass of 1.78g of acetylsalicylic acid was recovered. What is the experimental yield for its synthesis? Express the yield with the correct number of significnnt figures. 2. Experimental Procedure, Part A.5. Recrystallizing the aspirin removes some (or all) of the impurities in the sample. Explain how the recrystallization process performs this function. 3. Experimental Procedure, Part B.3. The melting point of the prepared aspirin in this experiment will most likely be less than (but not greater than) that of pure aspirin. Explain. See Experiment 14. 5. Experimental Procedure, Part C.I a. Determine the number of grams of acetylsalicylic acid that will react with 20.0mL of 0.100MNaOH. Show calculation here and on the Report Sheet. b. An aspirin sample was synthesized and analyzed. The dua for the analysis for Trial I is in the table below. (See Report Sheet.) From the data detennine the percent purity of the apirin sunple. Record calculated values with the comect number of significant figures. Calculation Zone c. For Trials 2 and 3 , the percent purity was detemined to be 94.5% and 93.95 respectively. a. What is the avenge percent purity of the aspirin sample? b. What are the standard deviation and the relative standard deviation (\%RSD) for the percent purity of the aspirin sample