To calculate the reaction is reactant or product favored at equliribrium at 298 K and the reaction is more or less product favored at higher temperature. Concept introduction: The Δ S ∘ ( system ) can be calculated by the following expression, Δ S ∘ ( system ) = Δ r S ° = ∑ n S ° ( products ) − ∑ n S ° ( reactants ) Enthalpy of formation of the reaction can be calculated by following expression, Δ r H ° = ∑ n Δ f H ° ( products ) − ∑ n Δ f H ° ( reactants ) The Gibbs free energy or the free energy change is a thermodynamic quantity represented by Δ G ∘ . It is related to entropy and entropy by the following expression, Δ G ∘ = Δ H ∘ − T Δ S ∘ Here, Δ r H ∘ is the enthalpy change for the reaction. If the value of Δ r G ∘ is negative the reaction is product favored at equilibrium at 298 K .
To calculate the reaction is reactant or product favored at equliribrium at 298 K and the reaction is more or less product favored at higher temperature. Concept introduction: The Δ S ∘ ( system ) can be calculated by the following expression, Δ S ∘ ( system ) = Δ r S ° = ∑ n S ° ( products ) − ∑ n S ° ( reactants ) Enthalpy of formation of the reaction can be calculated by following expression, Δ r H ° = ∑ n Δ f H ° ( products ) − ∑ n Δ f H ° ( reactants ) The Gibbs free energy or the free energy change is a thermodynamic quantity represented by Δ G ∘ . It is related to entropy and entropy by the following expression, Δ G ∘ = Δ H ∘ − T Δ S ∘ Here, Δ r H ∘ is the enthalpy change for the reaction. If the value of Δ r G ∘ is negative the reaction is product favored at equilibrium at 298 K .
Solution Summary: The author explains that the Gibbs free energy is a thermodynamic quantity represented by DeltaGcirc.
Science that deals with the amount of energy transferred from one equilibrium state to another equilibrium state.
Chapter 21, Problem 91GQ
Interpretation Introduction
Interpretation:
To calculate the reaction is reactant or product favored at equliribrium at 298 K and the reaction is more or less product favored at higher temperature.
Concept introduction:
The ΔS∘(system) can be calculated by the following expression,
ΔS∘(system)=ΔrS°=∑nS°(products)−∑nS°(reactants)
Enthalpy of formation of the reaction can be calculated by following expression,
ΔrH°=∑nΔfH°(products)−∑nΔfH°(reactants)
The Gibbs free energy or the free energy change is a thermodynamic quantity represented by ΔG∘. It is related to entropy and entropy by the following expression,
ΔG∘=ΔH∘−TΔS∘
Here, ΔrH∘ is the enthalpy change for the reaction.
If the value of ΔrG∘ is negative the reaction is product favored at equilibrium at 298 K.
Given the overall reaction from the previous problem:
2 CO (g) + 6 H2 (g) D 2 CH4 (g) + 2 H2O (g)
Using Le Chatelier’s principle, predict which direction the reaction will shift to reestablish equilibrium for each of the following changes:
Calculate the enthalpy of reaction for this reaction using the standard thermodynamics values for the reactants and products. Is the reaction endothermic or exothermic?
Now, use Le Chatelier’s principle again to determine the direction the equilibrium will shift if heat is added to the reaction.
If 35 kPa of CO is mixed with 35 kPa of hydrogen in a 1.5 L container at 25°C, what is the theoretical yield of methane?
= 40 kJ/mol, decide if the following statement is true. If the statement is false,
For a reaction with AH
choose the statement that makes it true. Select the single best answer.
The product is favored at equilibrium. (Assume the entropy term is small compared to the enthalpy
term)
The statement is false. Neither the product nor the starting material is favored at equilibrium.
The statement is false. The equilibrium position of the reaction cannot be approximated.
The statemnent is true.
The statement is false. The starting material is favored at equilibrium.
1. Write the ΔHf˚ reaction for HNO3, accounting for the enthalpy term in your reaction.
2. Is the reaction more likely to be thermodynamically favorable at 25 °C or 95 °C? Justify your answer.
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