What effect do the listed changes have on the position of the equilibrium in the reaction of carbon with hydrogen? C(s) + 2 H 2 (g) ⇌ CH 4 (g) ∆ H = -18 kcal/mol (-75kJ/mol) c. Allowing CH 4 to escape continuously from the reaction vessel

Hello everyone today. We have the following problem. How will the change below affect the direction of equilibrium in the falling reaction between sulfur and oxygen gas? Sulfur trioxide produced is continuously collected in a separate container. So our sulfur trioxide is a product in this reaction. So we can say that if we remove our sulfur trioxide, the reaction is going to shift in the direction that will replace it. So the reaction will shift to the right to produce more to produce more. And that is because the concentrations of our sulfur trioxide will will decrease. So the direction of the equilibrium will be a shift to the right to produce more sulfur dioxide. And with that we have answered the question overall, I hope this helped, and until next time.

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1. Matter and Measurements4h 31m
2. Atoms and the Periodic Table5h 23m
3. Ionic Compounds2h 18m
4. Molecular Compounds2h 18m
5. Classification & Balancing of Chemical Reactions3h 17m
6. Chemical Reactions & Quantities2h 27m
7. Energy, Rate and Equilibrium3h 46m
8. Gases, Liquids and Solids3h 25m
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11. Nuclear Chemistry56m
BONUS: Lab Techniques and Procedures1h 38m
BONUS: Mathematical Operations and Functions47m
12. Introduction to Organic Chemistry1h 34m
13. Alkenes, Alkynes, and Aromatic Compounds2h 12m
14. Compounds with Oxygen or Sulfur1h 6m
15. Aldehydes and Ketones1h 1m
16. Carboxylic Acids and Their Derivatives1h 11m
17. Amines39m
18. Amino Acids and Proteins1h 51m
19. Enzymes1h 37m
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26. Nucleic Acids and Protein Synthesis2h 54m

7. Energy, Rate and Equilibrium

Le Chatelier's Principle

GOB Chemistry

7. Energy, Rate and Equilibrium

Le Chatelier's Principle

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Problem 16c

Textbook Question

What effect do the listed changes have on the position of the equilibrium in the reaction of carbon with hydrogen?
C(s) + 2 H₂(g) ⇌ CH₄(g) ∆H = -18 kcal/mol (-75kJ/mol)
c. Allowing CH₄ to escape continuously from the reaction vessel

Verified step by step guidance

Identify the type of reaction: The reaction is exothermic (∆H = -18 kcal/mol), meaning it releases heat as it proceeds in the forward direction.

Understand the equilibrium principle: According to Le Chatelier's Principle, if a change is made to a system at equilibrium, the system will adjust to counteract that change and restore equilibrium.

Analyze the effect of CH4 escaping: If CH4 (a product) is continuously removed from the reaction vessel, the concentration of CH4 decreases. This disrupts the equilibrium by reducing the product concentration.

Predict the shift in equilibrium: To counteract the removal of CH4, the equilibrium will shift to the right (toward the products) to produce more CH4 and restore balance.

Conclude the effect: Allowing CH4 to escape continuously will drive the reaction forward, increasing the consumption of C(s) and H2(g) to produce more CH4(g).

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change. In the context of the given reaction, allowing CH4 to escape continuously reduces its concentration, prompting the equilibrium to shift to the right to produce more CH4, thereby attempting to restore balance.

Equilibrium Position

The equilibrium position of a reaction refers to the relative concentrations of reactants and products at equilibrium. In the reaction C(s) + 2 H2(g) ⇌ CH4(g), the position can be influenced by changes in concentration, pressure, or temperature. Understanding how these factors affect the equilibrium position is crucial for predicting the outcome of the reaction when CH4 is allowed to escape.

Endothermic and Exothermic Reactions

Reactions can be classified as endothermic or exothermic based on heat exchange. The given reaction is exothermic (∆H = -18 kcal/mol), meaning it releases heat. This characteristic is important because changes in temperature can also affect the equilibrium; for exothermic reactions, increasing temperature shifts the equilibrium to favor reactants, while decreasing temperature favors products.

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The reaction CO(g) + H₂O(g) ⇌ CO₂(g) + H₂(g) has ∆H = -9.8 kcal/mol (-41 kJ/mol). Does the amount of H₂ in an equilibrium mixture increase or decrease when the temperature is decreased?