exothermic and endothermic.
- a. Define the terms exothermic and endothermic. In a calorimetric experiment,how does on determine whether a reaction is one or the other?
b. In a calorimetric experiment, why is it important to determine the heat capacity of the calorimeter?
2. Two solutions namely, 500 mL of 0.50 M HCl and 500 mL of 0.50 M NaOH at the same temperature of 21.6o C are mixed in a constant-pressure calorimeter. The heat capacity of the calorimeter was 450 J/oC. Given that the specific heat of the solution is 4.184 J/goC, the density of the solution is 1.00 g/mL, and that the heat of neutralization for the process H+ (aq) + OH- (aq) -> H2O (l) is -56.2 kJ, what is the final temperature of the mixed solution?
3. You are given the following standard enthalpies of formation at 25oC.
NH4OH (aq) -80.29 kJ/mol,
H+Â (aq) 0 kJ/mol,
NH4+Â (aq) -132.5 kJ/mol,
H2O (l) -285.85 kJ/mol
a. Calculate the standard enthalpy of neutralization of NH4OH (aq)
NH4OH (aq) + H+Â (aq) -> NH4+Â (aq) + H2O (l)
b. Using the value of -56.2 kJ/mol as the standard enthalpy change for the reaction: H+Â (aq) + OH-Â (aq) -> H2O (l)
calculate the standard enthalpy for the reaction: NH4OH (aq) -> NH4+Â (aq) +OH-Â (aq)
Â
4. You are given the following information:
CO (g) + 1/2 O2 (g) -> CO2 (g) Hof = -283.0 kJ
N2 (g) + O2 (g) -> 2 NO (g) Hof = +180.6 kJ
Determine the standard enthalpy change for the reaction:
CO (g) + NO (g) -> CO2Â (g) + 1/2 N2Â (g) /_ H = ?
Answers
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Posted 27 Apr 2017 04:04 AM
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