Factors That Affect Reaction Rates Lab 11a

Factors That Affect Reaction Rates Lab 11A

Introduction:

The point of this experiment is to analyze and understand how changing (increasing and decreasing) temperature, surface area and concentration affect the reaction rate.

Procedure:

Part 1:

Obtain 8 cm of Mg ribbon from teacher + record given a mass of 1.000m of the ribbon in your copy of Table 1

Cut Mg into eight strips 1.00cm long

Label 4 test tubes with an appropriate concentration of hydrochloric acid to be added (0.5M, 1.0M, 3.0M, and 6.0M)

With a graduated cylinder, measure 10mL of each of the concentrations of acid in the appropriate test tubes

Place the Mg strips in the test tubes. Start timing as soon as the Mg comes in contact with the acid. Measure time of the reaction.

After performing the analysis of results with a teacher, calculate the reaction rate.

Part 2:

Obtain four 250mL beakers and add 150mL water to each of about 100, 50, 20, and 0 degrees Celsius.

Place 10 mL of 1.0M hydrochloric acid into each of the four test tubes. Place each test tube in a beaker and wait 3-4 min to allow the solvent to become the temperature of the water.

Using the first test tube measure the temperature of the acid and record the value in table 2. Place one Mg strip in the acid and record the time took for the reaction.

Part 3:

Determine mass of CaCO3 chip and transfer is to a 250 mL erlenmeyer flask.

Using a watch or a clock that shows seconds, note the time as you add 15 mL of 3M HCL to the flask.

Notes the time to when the chip dissolves. If after five minutes the chip hasn't dissolved, pour off the acid in the reaction, rince the marble chip, and set it aside on a paper towel. Weight the chip before you leave the laboratory, recording results in table 3.

Using a piece of weighing paper, determine the exact mass of about 0.75g - 1.00g of powdered calcium carbonate, CaCO3, and transfer it to a 250mL Erlenmeyer flask.

Using a watch or clock that shows time in seconds, note the time as you add 15 mL of 3M HCL to the flask.

Again note the time when the reaction mixture stops bubbling and the powdered CaCO3 has dissolved. Record the elapsed time in your copy of the table 3.

Do not calculate Reaction Rate in Table 3 until you perform the