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1. Determine the mass of one mole (molar mass) of calcium chloride (CaCl2).
2. Calculate the mass of 0.030 moles of calcium chloride (CaCl2).
3. When 0.030 moles of calcium chloride was placed into 25.0 ml of water and the temperature was recorded every min. the following data was collected:
Time Temp (00C) Time Temp (00C) Time Temp (00C)
1 min 25.0 4 min 34.7 7 min 38.1
2 min 29.2 5 min 36.0 8 min 38.8
3 min 32.4 6 min 37.2 9 min 39.1
4. Graph this data. Give labels and units for both axes.
5. Is the dissociation exothermic or endothermic? How can you tell?
6. Using the temperatures from the data table, calculate and record T (highest temperature – starting temperature).
7. Calculate the heat exchanged in this process using the following equation:
Heat = masswater x T x 4.18j/goC (remember for water 1ml = 1g)
8. This amount of heat represents dissolving 0.030 moles of calcium chloride. Determine the amount of heat that would be involved in dissolving 1.0 moles.
9. Write the balanced equation for the dissociation of calcium chloride (CaCl2) in water. Include the heat term (determined in # 8) on the appropriate side of the equation.
10. Draw a model showing the aqueous Ca2+ and Cl- ions (the ions surrounded by water molecules) showing the correct orientation of water molecules around the cation and anion.
1. Trace the flow of electrons, Ca+2 and Cl-1 ions during the electrolysis of molten CaCl2.
2. Label the anode and cathode.
3. Write the anode and cathode half-reactions.
4. Indicate the substances formed at each electrode
5. Describe an application of electrochemistry.
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