At the beginning of this chapter we noted that the reaction of CO2 with H2 O to form a hydrocarb

Name: Problem 145, Chapter 18: Chemistry: The Molecular Nature of Matter
Uploaded: 2021-08-26T21:24:53-08:00
Duration: 1 min 29 s
Channel: David Collins
Description: At the beginning of this chapter we noted that the reaction of CO2 with H2 O to form a hydrocarbon fuel is nonspontaneous. According to thermodynamics, where would the position of equilibrium lie for such a reaction. Why?

step 1 Just because a reaction is non -spontaneous, meaning it has a negative delta G, does not mean it

Question

At the beginning of this chapter we noted that the reaction of $\mathrm{CO}_{2}$ with $\mathrm{H}_{2} \mathrm{O}$ to form a hydrocarbon fuel is nonspontaneous. According to thermodynamics, where would the position of equilibrium lie for such a reaction. Why?

   At the beginning of this chapter we noted that the reaction of $\mathrm{CO}_{2}$ with $\mathrm{H}_{2} \mathrm{O}$ to form a hydrocarbon fuel is nonspontaneous. According to thermodynamics, where would the position of equilibrium lie for such a reaction. Why?

Chemistry: The Molecular Nature of Matter

Neil D. Jespersen,… 7th Edition

Chapter 18, Problem 145

Instant Answer

Solved by Expert David Collins

08/26/2021

Step 1

A nonspontaneous reaction is one that does not favor the formation of products at the specified conditions. In terms of Gibbs free energy (ΔG), a nonspontaneous reaction has a positive ΔG value. Show more…

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At the beginning of this chapter we noted that the reaction of $\mathrm{CO}_{2}$ with $\mathrm{H}_{2} \mathrm{O}$ to form a hydrocarbon fuel is nonspontaneous. According to thermodynamics, where would the position of equilibrium lie for such a reaction. Why?

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Key Concepts

Gibbs Free Energy

Gibbs free energy is a thermodynamic potential that helps predict whether a reaction will occur spontaneously. If the change in Gibbs free energy (?G) for a reaction is positive, the process is nonspontaneous, meaning that the reactants are favored at equilibrium. This concept is central to determining reaction feasibility and direction.

Chemical Equilibrium

Chemical equilibrium refers to the state of a chemical reaction where the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products. For a nonspontaneous reaction with a positive ?G, the equilibrium position lies on the side of the reactants, indicating that the formation of the products is thermodynamically unfavorable under standard conditions.

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