The same idea can be applied to chemical reactions. Not all reactions go directly from reactants to products, sometimes there are other reactions that happen along the way. For example, let's evaluate the following reaction: Equation 1: CH4(g) + H2O(g) → CO(g) + 3H2(g) AH° = ?? Think of this reaction as your "destination" or final reaction, for which we want to figure out the change in enthalpy. We can use two separate reactions each with their own independent changes in enthalpy to calculate the unknown enthalpy for equation 1. Equation 2: CO(g) + H2(g) → C(s) + H2O(g) AH° =-131.3 kJ Equation 3: C(s) + 2H2(g) → CH«(g) AH° = 74.8 kJ
The same idea can be applied to chemical reactions. Not all reactions go directly from reactants to products, sometimes there are other reactions that happen along the way. For example, let's evaluate the following reaction: Equation 1: CH4(g) + H2O(g) → CO(g) + 3H2(g) AH° = ?? Think of this reaction as your "destination" or final reaction, for which we want to figure out the change in enthalpy. We can use two separate reactions each with their own independent changes in enthalpy to calculate the unknown enthalpy for equation 1. Equation 2: CO(g) + H2(g) → C(s) + H2O(g) AH° =-131.3 kJ Equation 3: C(s) + 2H2(g) → CH«(g) AH° = 74.8 kJ
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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.
Question
I’ve listed the equations in an image. not graded
Transcribed Image Text:3. In the space below rearrange equations 2 and 3 so that they do add up to your final reaction. Keep in
mind that you can flip, or reverse, the equation and you can multiply/divide the equation. However, whatever
you do to the equation you must also do to the AH®. (Hint: equations can be reversed, and quantities can be
increased or decreased by multiplying factors. Think about each substance as a variable.)
Equation 2:
Equation 3:
Equation 1:
CH«(g) + H2O(g) → CO(g) + 3H2(g)
AH° = ??
Transcribed Image Text:The same idea can be applied to chemical reactions. Not all reactions go directly from reactants to products,
sometimes there are other reactions that happen along the way. For example, let's evaluate the following reaction:
Equation 1:
CH4(g) + H2O(g) → CO(g) + 3H2(g)
AH° = ??
Think of this reaction as your "destination" or final reaction, for which we want to figure out the change in
enthalpy. We can use two separate reactions each with their own independent changes in enthalpy to calculate the
unknown enthalpy for equation 1.
Equation 2:
CO(g) + H2(g) → C(s) + H2O(g)
AH° =-131.3 kJ
Equation 3:
C(s) + 2H2(g) → CH4(g)
AH° = 74.8 kJ
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