5. Define catalyst. What is the catalyst in this lab? PURPOSE:• To synthesize esters and to identify the odor of each●To write chemical equations for the formation of each esterAPPARATUS AND MATERIALS:test tubes400 mL beakerhotplateSAFETY:Note: ethanoic acid I;is labelled Glacial Acetic AcidPROCEDURE:Lab - MAKING ESTERSdrop bottles of:Sulfuric acid is extremely corrosive. Avoid direct contact. If any touches your skin, wash it off immediately. Note theeyewash station.Alcohols and carboxylic acids are flammable. Use caution.TEST TUBEconcentrated sulfuric acidmethanolethanol1-octanolABCDE1. Prepare a hot water bath using the 400mL beaker and hotplate. Adjust the heating control to maintain a watertemperature of about 70°C.2. Label 5 test tubes A to F. Place the test tubes on a test tube rack3. In the appropriate test tube, add 0.5 mL (10 drops) of alcohol followed by 0.5 mL (10 drops) of the carboxylic acidaccording to the table below.CARBOXYLIC ACID0.25 g salicylic acid0.5 mL ethanoic acid0.5 mL butanoic acid0.5 mL ethanoic acid0.5 mL ethanoic acidbutanoic (butyric) acidn-pentanolsalicylic acid(solid)ALCOHOL0.5 mL methanolpentan-1-ol0.5 mL ethanol0.5 mL ethanol0.5 mL 1-octanol4. Add 4-5 drops of concentrated sulfuric acid to each test tube. (caution, it is corrosive!) I will add it for you5. Place the test tubes in a hot water bath (use 400 ml beaker with about 200 mL of water)and gently heat atapproximately 70 °C for 10 minutes.6. Cool the test tubes by immersing them in a cold water bath.7. Add 5 mL of tap water to each of the test tubes. The ester will form a layer above the water.8. Carefully note the odor of the contents of each test tube.9. Discard the contents of the test tubes in the large beaker in the fume hood at the back of the room.

The substance which usually increases the rate of reaction without itself being consumed during the…

Answered: 5. Define catalyst. What is the…

Science

Chemistry

5. Define catalyst. What is the catalyst in this lab?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Which would likely increase the rate of a chemical reaction? A. Cooling the reaction mixture. B. Decreasing the concentration of the reactants. C. Decreasing the surface area of the reactants. D. Adding a catalyst to the reaction mixture.
Reaction rate can NOT be increased by Question 17 options: adding an effective catalyst to the system decreasing the concentration of the reactants increasing the surface area of the reactants increasing the temperature of the system
5. What is the effect of a catalyst on a reaction? A. It increases the rate. B. It decreases the entropy. C. It changes the equilibrium. D. It makes the products more stable.
What is catalyst and their functions
17
8. Which of the following statements is the best explanation for the effect of increase in temperature on the rate of reaction? a. It increases the number of particles with the necessary activation energy b. It enables the reacting particles with the necessary activation energy c. It lowers the activation energy for the reaction d. It enables the activated complex to be more easily converted to the products
9. What are two factors that affect the kinetics of chemical reactions and were tested in the lab? Reactant concentration and temperature b. Catalyst and temperature c.. Reactant concertation and catalyst d. Physical state of reactant and catalyst e. Temperature and color с. the following
1. Find an example of a chemical system which is at steady state, and present it to the class. 2. Explain why it is at steady state and not at equilibrium. 3. Explain how this process is important to society. 4. Remember to provide all references used in proper APA citations with live links to your sources. Respond to two other classmates, and respond to substantial posts under your own thread.
Q1. According to the "collision theory" model, why does the rate of a reaction increase when temperature increases? I. There are more collisions per second. II. The molecules are vibrating with a higher frequency. III. A greater proportion of the collisions between reactants have the required activation energy for the reaction to proceed a. I only b. II only c. III only d. I,II and III e. I and III only Q2. A reaction was found to be first order with a rate constant of3.4×10−4 s−1What percentage of the starting material would remain after 2 hours? a.8.65%b.96.0%c.90.3%d.4.00%e.99.9%Q3. The half-life of a rection was calculated at 300 seconds. What \% of starting material would remain after 900 seconds? a.25%
QUESTION 4 Which of the following statements is TRUE about catalysts- a. They lower the Ea for at least one step in a chemical. reaction mechanism. Ob. Catalysts help a reaction to form a higher yield of products. Oc. C. They lower the AH for at least one step in the reaction mechanism. Cd. Catalysts have to be in the same phase as the reagents to be effective.
5. Consider a general reversible reaction: A+B- X+Y and answer the following questions. a. Describe what happens at equilibrium in terms of reaction rate and chemical concentrations? b. Write the expression for the equilibrium constant for the given reaction. 6. Consider the following general reversible reaction is taking place in a reaction vessel and has achieved a state of chemical equilibrium. A+2B 2X If the following stresses are applied to this reaction at equilibrium, which direction (forward or backward) will the equilibrium shift? a. Increase in concentration of A B. Decrease in concentration of X Factors Affecting Reaction Rate, Chemical Equilibrium and Le Chatelier's Principle MAY tv
1. a. Explain in your own words, what is meant by the term "activation energy." b. How can the idea of activation energy be used to explain the temperature dependance of rate? c. How can activation energy be used to explain why a catalyst increases the rate of a chemical reaction