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1. Define exothermic and endothermic reactions in terms of (a) the sign of ?H and (b) the temperature change for the reaction solution. 2. Define (a) heat capacity and (b) specific heat capacity. 3. A 650.0 mL sample of water was cooled from 60.5
°
C to 15.3
°
C. Calculate the value of q for this process. 4. A piece of metal with a mass of 6.45 g at 52.8
°
C is placed in a calorimeter containing 55.00 mL of water at 23.4
°
C. The final temperature of the mixture was recorded as 31.0
°
C. What is the specific heat of the metal? Assume that the calorimeter is perfect. 5. When a 4.75 g sample of solid KOH is dissolved in a calorimeter containing 75.00 g of water, the temperature increases from 20.78
°
C to 35.71
°
C. If the calorimeter has a heat capacity of 12.4 J/
°
C, calculate ?H (in kJ/molKOH ) for the solvation process KOH(s)?K
+
(aq)+OH
-
(aq). Assume that the specific heat of the solution is the same as water.1.
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