1. A student conducts an investigation to determine the heat of neutralization when 60.0 mL of 0.500 M sulfuric acid is reacted with 50.0 mL of 1.00 M sodium hydroxide. The following lab data was collected. • initial temperature of NaOH 23.4°C • initial temperature of H2SO4 23.4°C • stabilized temperature of mixture 29.3 °C a. What sign would ΔHneut have for this reaction? Is neutralization an exothermic or endothermic reaction? Explain. b. Assuming that the calorimeter has a specific heat capacity of 1.0 × 101 J/°C and that the density and specific heat capacity of the solution are the same as that of water, calculate the heat of neutralization for this reaction (q). c. Calculate the molar enthalpy of solution (ΔHneut) for this reaction.
Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
1. A student conducts an investigation to determine the heat of neutralization when 60.0 mL of 0.500 M sulfuric acid is reacted with 50.0 mL of 1.00 M sodium hydroxide. The following lab data was collected. • initial temperature of NaOH 23.4°C • initial temperature of H2SO4 23.4°C • stabilized temperature of mixture 29.3 °C
a. What sign would ΔHneut have for this reaction? Is neutralization an exothermic or endothermic reaction? Explain.
b. Assuming that the calorimeter has a specific heat capacity of 1.0 × 101 J/°C and that the density and specific heat capacity of the solution are the same as that of water, calculate the heat of neutralization for this reaction (q).
c. Calculate the molar enthalpy of solution (ΔHneut) for this reaction.
d. Explain how the heat of neutralization (q) and molar enthalpy of neutralization (ΔHneut) would change if the molarities of the solutions were both doubled.
e. If a significant amount of heat were lost to the air during the experiment, how would this affect the calculated molar enthalpy of neutralization? Explain.
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