Pour the solution in the calorimeter into a large beaker to combine with the

Pour the solution in the calorimeter into a large

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Pour the solution in the calorimeter into a large beaker to combine with the other part and neutralize. Part D: Enthalpy of Neutralization of Solid NaOH 19. Measure 50.0 mL of 1M HCl and 2.0 g of NaOH 20. Read the temperature of the HCl at 1-minute intervals for 3 minutes. 21. At the three minute mark, quickly pour the NaOH into calorimeter A and stir thoroughly 22. Continue reading the temperature for another 6 minutes at 1 minute intervals 23. Pour the solution in the calorimeter into a large beaker to combine with the other part and neutralize. Clean Up 24. Neutralize of the solutions from parts B-D to a PH between 6 and 8. Add HCl if the solution is basic and add sodium bicarbonate if the solution is acidic. RESULTS/DISCUSSION 1. Calorimeter Constant (Part A) 2. Enthalpy of Neutralization (Part B) 3. Enthalpy of Solution (Part C) 4. Enthalpy of Solution and Neutralization (Part D) 5. Hess’s Law
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CONCLUSION This lab successfully allowed students to investigate the quantity of energy transferred by heat (q 0 ) for chemical reactions. We were also quantitatively able to determine the enthalpy change for several chemical reactions and compare them to one another and sum reactions in order to obtain the enthalpy of another. Doing so, we were able to prove the validity of Hess’s Law of Constant heat summation,
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