Question

10. When sodium chloride dissolves in water, the ions dissociate: NaCl (s) = Na⁺ (aq) + Cl^- (aq)

AGO no spontaneous; RattaMY FAUNED AG. o o equilibrium secase rules toodeds React = Formation of mactats formation of prodrets AGLO i exothermie o speadanios product Favored 66-30-20 stultz Jenny unless you input energy 3-13: The Balance Between Enthalpy and Entropy For chemical reactions, we say that a reaction proceeds to the right when AG is negative and that the reaction proceeds to the left when AG is positive. At equilibrium AG is zero. The Gibbs-Helmholtz equation specifies that at constant temperature AG=AH - TAS or, in other words, that the sign and size of AG is governed by the balance between enthalpic (AH) and entropic (A$) considerations. In this assignment, you will dissolve several different salts in water, measure the resulting temperature changes, and then make some deductions about the thermodynamic driving forces behind the dissolving process. 1. Start Virtual ChemLab, select Thermodynamics, and then select The Balance Between Enthalpy and Entropy from the list of assignments. The lab will open in the Calorimetry laboratory. 2. There will be a bottle of sodium chloride (NaCl) on the lab bench. A weigh paper will be on the balance with approximately 2 g of NaCl on the paper. 2,0718 3. The calorimeter will be on the lab bench and filled with 100 ml water. Click on the Lab Book to open it. Make certain the stirrer is On (you should be able to see the shaft rotating). In the thermometer window click Save to begin recording data. Allow 20-30 seconds to obtain a baseline temperature of the water. sample 4. Drag the weigh paper with the sample to the calorimeter until it snaps into place and then pour the the calorimeter. Observe the change in temperature until it reaches a maximum (or minimum) and then record data for an additional 20-30 seconds. (You can click the clock on the wall labeled Accelerate to accelerate the time in the laboratory.) Click Stop. A data link icon will appear in the Lab Book. Click the data link icon and record the temperature before adding the NaCl and the highest or lowest temperature after adding the NaCl in the data table. 250c 5. Click the red disposal bucket to clear the lab. Click on the Stockroom to enter. Click on the clipboard and select the preset experiment called Heat of Solution-NaNO3 and repeat the experiment with NaNO3. Record the initial and final temperatures in the data table. 24.8000 6. Click the red disposal bucket to clear the lab. Click on the Stockroom to enter. Click the clipboard and select the preset experiment called Heat of Solution-NaAc and repeat the experiment with NACH:CO2 (NaAc). Record the initial and final temperatures in the data table. Data Table AT ("C) Mixture 20178g NaCl + H200 1.48449 NaNO3 + H2002 1.94347 NaCH;CO2 (+ H200 T. (°C) 25oC 22.9°C 25°C T2(°C) २५.१८ 24.०८न्ट 25,854C .0.440C + 0,88°C eyo erd endo Use your experimental data to answer the following questions: 7. Calculate AT for each mixture and record the results in the data table. AT-T2-T 8. An exothermic process releases heat (warms up), and an endothermic process absorbs heat (cools down). Beyond Labz, all rights reserved

Write ionic equations, similar to the one above, that describe how NaNO₃ and NaCH₃CO₂ each dissociate as they dissolve in water. Include heat as a reactant or product in each equation.

Here is what I answered:

NaNO_{3 (s)} = Na⁺ + NO₃^-  + heat

NaC₂H₃O₂ + Heat = Na⁺ + C₂H₃O₂^-_(ag)

Lab data table attached to determine where to place heat.

Answer 1