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Does the equilibrium favor the reactant or the products? Choose one: products neither reactants There is no way to tell Where is the equilibrium position on the graph? Choose one: At the lowest point in the curve At the highest point in the curve on the left (reactant side) Halfway between the reactants and products At the highest point in the curve on the right (product side)

Does the equilibrium favor the reactant or the products? Choose one: products neither reactants There is no way to tell Where is the equilibrium position on the graph? Choose one: At the lowest point in the curve At the highest point in the curve on the left (reactant side) Halfway between the reactants and products At the highest point in the curve on the right (product side)

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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Consider the gas-phase reaction of hydrogen and iodine at 298.15 K and the graph showing the free energy of the H2-I2-HI mixture.

H2​(g)+I2​(g)⇌2HI(g)

Does the equilibrium favor the reactant or the products?

Choose one:

products

neither

reactants

There is no way to tell

Where is the equilibrium position on the graph?


Choose one:

At the lowest point in the curve

At the highest point in the curve on the left (reactant side)

Halfway between the reactants and products

At the highest point in the curve on the right (product side)

The image depicts a graph illustrating the change in Gibbs free energy (ΔG°) for a chemical reaction. The vertical axis represents Gibbs free energy (G), while the horizontal axis is not labeled with specific variables. The curve on the graph shows a downward trend, indicating a decrease in Gibbs free energy as the reaction progresses. Key points on the graph are highlighted: 1. At the start of the reaction: - ΔG° is noted as -54.226 kJ for the formation of 1 mole of H₂ and 1 mole of I₂. 2. At the end of the reaction: - ΔG° is -70.234 kJ for the formation of 2 moles of HI. These values imply that the reaction is exergonic, releasing energy as it proceeds towards the formation of hydrogen iodide (HI) from hydrogen (H₂) and iodine (I₂) in their standard states. The greater magnitude of ΔG° at the end highlights a more stable product formation.
Transcribed Image Text:The image depicts a graph illustrating the change in Gibbs free energy (ΔG°) for a chemical reaction. The vertical axis represents Gibbs free energy (G), while the horizontal axis is not labeled with specific variables. The curve on the graph shows a downward trend, indicating a decrease in Gibbs free energy as the reaction progresses. Key points on the graph are highlighted: 1. At the start of the reaction: - ΔG° is noted as -54.226 kJ for the formation of 1 mole of H₂ and 1 mole of I₂. 2. At the end of the reaction: - ΔG° is -70.234 kJ for the formation of 2 moles of HI. These values imply that the reaction is exergonic, releasing energy as it proceeds towards the formation of hydrogen iodide (HI) from hydrogen (H₂) and iodine (I₂) in their standard states. The greater magnitude of ΔG° at the end highlights a more stable product formation.
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