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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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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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: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° = ??
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
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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