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Understanding Single Replacement Reactions: Exothermic and Endothermic Processes

This document explores single replacement reactions (SRR), where a free element replaces a less active element in a compound. It highlights the characteristics of these reactions, demonstrating with examples and emphasizing the energy changes involved—exothermic (energy released) and endothermic (energy absorbed). Included are hands-on lab activities using hydrochloric acid and various metals to visualize these reactions and their thermal effects. Participants will record observations and balance chemical equations, enriching their understanding of chemical reactivity and thermodynamics.

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Understanding Single Replacement Reactions: Exothermic and Endothermic Processes

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  1. IAN pg. 50 REACTIONS Single Replacement, Exothermic, Endothermic.

  2. Single Replacement Reactions • SRR: reaction where a free element replaces a less active element in a compound • SR Reactions always start and end with an element and a compound • Example: Zn + CuSO4 ZnSO4 + Cu

  3. Exo-/Endo- Thermic • Chemical Reactions always involve energy: • Exothermic: energy is released • Endothermic: energy is absorbed • Endothermic reactions usually “feel cold”

  4. Lab Activity: SRRPart A • Pour about 1/2 inch of HCl into each of the 4 test tubes. • Place one of the metals into a test tube. • Feel the bottom of each tt as the reaction proceeds and note any other observations in the data table. Observe for 5 minutes. • When finished, pour off the acid into the sink and rinse any metals that are left with water and put them back into the tray.

  5. IAN pg. 49. DATA TABLEPart A Do the observations UNDER the lab directions for Part A Hydrochloric Acid (HCl) mixed with: magnesium (strip):____________________ aluminum (tiny pieces):________________ zinc (pinch of powder):________________ copper (wire):_______________________

  6. Lab Activity: Endothermic Reaction, Part B • Place small spoonfuls of calcium chloride (CaCl2) and baking soda into a baggie. • Put the powders into a corner of the baggie and twist it. • Into the other corner of the baggie, pour a small amount of water. • Press the air out and close the baggie. • Mix the contents together and feel the resulting mixture for temperature change. Record your observations.

  7. OBSERVATIONSPart B Record what you observed when the calcium chloride, baking soda, and water were mixed inside the baggie (a closed system):

  8. CONCLUSIONS • Write the single replacement reaction equations: a. Magnesium and HCl b. Aluminum and HCl c. Zinc and HCl • Were they exothermic or endothermic? • Which metal(s) are more active and which are less active than hydrogen? • Balance the SRR equation: AgNO3 + Cu  Cu(NO3)2 + Ag

  9. SRR Equations 2HCl + Mg  MgCl2 + H2 6HCl + 2Al  2AlCl3 + 3H2 6HCl + 2Zn  2ZnCl3 + 3H2

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