Consider the decomposition of liquid hydrogen peroxide (H2O2) to form water and oxygen.a. What is the heat of formation for hydrogen peroxide?b. What is the heat of formation for liquid water?c. What is the heat of formation for gaseous oxygen? Why?d. Write the balanced chemical equations that correspond to the ΔH values you looked up for parts a, b, and c.e. Write the balanced chemical equation for the decomposition of hydrogen peroxide to form water and oxygen. (Write the equation such that the coefficient on oxygen is 1.)f. What is the heat of reaction for the process in part e?g. Draw a scale diagram of this reaction (1 cm = 100 kJ) that shows the relative energies of reactants (on the left), products (on the right), and the elements in their most stable states (in the middle). Label all the energies you know.
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.
Consider the decomposition of liquid hydrogen peroxide (H2O2) to form water and oxygen.
a. What is the heat of formation for hydrogen peroxide?
b. What is the heat of formation for liquid water?
c. What is the heat of formation for gaseous oxygen? Why?
d. Write the balanced chemical equations that correspond to the ΔH values you looked up for parts a, b, and c.
e. Write the balanced chemical equation for the decomposition of hydrogen peroxide to form water and oxygen. (Write the equation such that the coefficient on oxygen is 1.)
f. What is the heat of reaction for the process in part e?
g. Draw a scale diagram of this reaction (1 cm = 100 kJ) that shows the relative energies of reactants (on the left), products (on the right), and the elements in their most stable states (in the middle). Label all the energies you know.
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