chemistry week 6 lab

Topics: Thermodynamics, Chemical reaction, Energy, Temperature, Heat / Pages: 3 (505 words) / Published: May 11th, 2015
Laboratory 6: Energy Changes in Chemical Reactions
Note: Lab reports are to be completed by each student individually and in their own words
Observations: (This part is to be completed in class)
Part 1: Physical Change- Heat of Solution for Sodium hydroxide (NaOH)
3.2 grams NaOH
Temperature of DI water = ____22.8 °C
Temperature after addition of NaOH = ______31.8 °C
Part 2: Chemical Change- Reaction between acid and base
Temperature of HCl = ___21.4 °C
Temperature after addition of pellets of NaOH = ____26.4 °C
Part 3: Chemical Change- Reaction between stomach acid and antacid
Temperature of HCl = __23.3 °C
Temperature after addition of Tums = __18.5 °C

Questions and Conclusions:
This part (everything below) is to be completed by each student individually in their own words. Plagiarism or copying will be penalized.
Part 4: General Concepts- Define the following Terms
Exothermic Reaction: are chemical reactions that are letting go energy with heat, light, or sound are impulsive.

Endothermic Reaction: chemical reactions that have to take in energy in order to work and are not impulsive.

First Law of Thermodynamics: basically means matter or energy can not be created or destroyed. The universe is energy endless, it can be changed, moved, controlled, stored, or dissolute.

Second Law of Thermodynamics: Increased Entropy; the quality of matter and energy declines progressively over time.

Part 5. Answer the following questions:
1. If ice is added to hot water, how will the energy change? Why?
When you have a glass22 of hot water and add ice, it will cool down. There will be an exchange of heat energy that will come from the hot water to the ice. This type of exchange will cause the ice to melt and cool the hot water.

Part 6: Conclusion
Write the results in the table 1 and calculate difference in temperature.
Table 1:
Initial Temperature
Final Temperature
Change in Temperature= Final temperature-Initial temperature

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