1. Ensure that the calorimeter vial used in Part A is clean and dry.
2. Assemble the calorimeter as shown in Figure B2.2. Pour the entire contents of the bottle of pre-measured 20 mL of hydrochloric acid (1 mol ⋅ L−1) into the vial. Ensure that the thermometer bulb is below the surface of the liquid, and determine the temperature of the hydrochloric acid.
3. Pour the entire contents of one of the pre-weighed vials of magnesium powder (approximately 0.12 g) into the hydrochloric acid contained in the calorimeter. Stir the mixture vigorously, taking care not to hit the thermometer with the stirrer. Read the temperature of the reaction mixture every 15 seconds, until it reaches a maximum. Thereafter, read the temperature every minute for five minutes.
4. Check the contents of the calorimeter. If all the magnesium did not dissolve, you must start Part B again.
5. Dispose of the contents of the calorimeter vial down the drain with plenty of water. Wash the vial with water, and dry it with tissues or paper towels.
6. Repeat steps 1 though 5 for a second determination.
Magnesium Oxide Reaction
1. Set up the calorimeter as before. Again pour the entire contents of the bottle of pre-measured 20 mL of hydrochloric acid (1 mol ⋅ L−1) into the calorimeter vial, and measure the temperature of the acid.
2. Pour the entire contents of one of the pre-weighed vials of magnesium oxide (approximately 0.25 g) into the hydrochloric acid contained in the calorimeter, stir thoroughly, and monitor the temperature change in exactly the same manner as you did in step 3, above.
3. Check the contents of the calorimeter.
If you can see any unreacted magnesium oxide you must repeat the experiment.
4. Dispose of the contents of the calorimeter down the drain. Wash the cup with water, and dry it with paper towels or tissues.
5. Repeat steps 1 through 4 for a second determination.
These solutions may offer step-by-step problem-solving explanations or good writing examples that include modern styles of formatting and construction of bibliographies out of text citations and references. Students may use these solutions for personal skill-building and practice. Unethical use is strictly forbidden.Laboratory Report Experiment B2
Title: Determination of Enthalpy Change
Purpose: The purpose of this lab is to understand enthalpy change and its calculation using calorimeter. In some cases where directly enthalpy cannot be determined so in such case learns to use Hess’s Law for the same.
Procedure:The experiment was conceded ready as drew in Experiment B2 of Chemistry 217 Home Lab Manual, pp. 155-170.
Part A. Find out heat capacity of Calorimeter
I observed that heat is released and water gets cooled and temperature decreased after addition of hot water to cold water.
Part B. find out Enthalpy of Magnesium Oxide formation
I observed that heat is absorbed and the temperature was increased after addition of Mg to Aq HCl.
I also observed that heat is absorbed and the temperature was increased after addition of MgO to Aq HCl.
Results & Calculations:
The results of the experiment discussed below as follows:...
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