Consider the reaction C12H22O11(s) + 1202 (g)→12CO2(g) +11H2O(1) in which 10.0 g of sucrose, C12H22011, was burned in a bomb calorimeter with a heat capacity of 7.50 kJ/°C. The temperature increase inside the calorimeter was found to be 22.0 °C. Calculate the change in internal energy, AE, for this reaction per mole of sucrose. Express the change in internal energy in kilojoules per mole to three significant figures.
Consider the reaction C12H22O11(s) + 1202 (g)→12CO2(g) +11H2O(1) in which 10.0 g of sucrose, C12H22011, was burned in a bomb calorimeter with a heat capacity of 7.50 kJ/°C. The temperature increase inside the calorimeter was found to be 22.0 °C. Calculate the change in internal energy, AE, for this reaction per mole of sucrose. Express the change in internal energy in kilojoules per mole to three significant figures.
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Chapter6: Thermochemisty
Section: Chapter Questions
Problem 6.132QP
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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.
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Transcribed Image Text:Consider the reaction
C12 H22O11 (s) + 1202(g)→12CO2(g) + 11H20(1)
in which 10.0 g of sucrose, C12H22011, was burned in a bomb calorimeter with a heat capacity of 7.50 kJ/°C. The temperature increase inside
the calorimeter was found to be 22.0 °C. Calculate the change in internal energy, AE, for this reaction per mole of sucrose.
Express the change in internal energy in kilojoules per mole to three significant figures.
Transcribed Image Text:A calorimeter is an insulated device in which a chemical
reaction is contained. By measuring the temperature change,
AT, we can calculate the heat released or absorbed during
the reaction using the following equation:
q= specific heat x mass x AT
Or, if the calorimeter has a predetermined heat capacity, C,
the equation becomes
q=C x AT
At constant pressure, the enthalpy change for the reaction,
AH, is equal to the heat, qp; that is,
AH= 4p
but it is usually expressed per mole of reactant and with a
sign opposite to that of q for the surroundings. The total
internal energy change, AE (sometimes referred to as
AU), is the sum of heat, q, and work done, w:
AE=q+w
However, at constant volume (as with a bomb calorimeter)
w =0 and so AE= qv-
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