CHM

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CHM 101 Module Four Additional Homework Problems 1. In order to verify the heat of reaction, a chemist mixes 1 liter of 1 M NaOH and 1 liter of 1 M HCl. The initial temperature of the two solutions is 25 C. The specific heat of water is 4.184 J/g C. The enthalpy of reaction of the following is –58 kJ/mol. HCl(aq) + NaOH(aq) NaCl(aq) + H 2 O(l) a) Is this reaction exothermic or endothermic? (Will the temperature increase or decrease?) The reaction is exothermic due to the negative change in enthalpy. b) Considering only the specific heat of the 2 liters of water and no heat transfer to/from surroundings, what is the final temperature of the solution (notice that the specific heat is in terms of mass, not volume)? -58kJ/mol = (-58 x 10 3 )(1mol)/(4.184J/mol C)/(2000g) = -6.93 C change 25 C – (-6.93) = 31.93 C 2. The same reaction takes place in two different vessels, which are initially at atmospheric pressure (1 atm). The first vessel is rigid and does not expand with change in pressure; the second vessel will expand to maintain a pressure of 1 atm inside. Over the course of a reaction, the second vessel expands by 1 liter.

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