Table of contents

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
9. Solutions4h 10m
10. Acids and Bases3h 29m
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
20. Carbohydrates1h 41m
21. The Generation of Biochemical Energy2h 8m
22. Carbohydrate Metabolism2h 22m
23. Lipids2h 26m
24. Lipid Metabolism1h 45m
25. Protein and Amino Acid Metabolism1h 37m
26. Nucleic Acids and Protein Synthesis2h 54m

7. Energy, Rate and Equilibrium

Rate of Reaction

GOB Chemistry

7. Energy, Rate and Equilibrium

Rate of Reaction

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0:54 minutes

Problem 76c

Textbook Question

How would each of the following change the rate of the reaction shown here?
2 NO(g) + 2 H₂(g) → N₂(g) + 2 H₂O(g)
c. removing some H₂(g)

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Identify the factors that influence the rate of a chemical reaction. These include concentration of reactants, temperature, presence of a catalyst, and surface area (if applicable). In this case, we are focusing on the concentration of H₂(g).

Understand the role of H₂(g) in the reaction. According to the balanced equation, H₂(g) is a reactant, and its concentration directly affects the reaction rate based on the collision theory. Fewer H₂ molecules mean fewer collisions with NO molecules.

Apply the concept of the rate law. The rate law for this reaction would depend on the concentrations of the reactants. If the reaction is second-order with respect to H₂(g), the rate would be proportional to [H₂]². Removing some H₂ would decrease its concentration, thereby reducing the reaction rate.

Consider the effect of removing H₂(g) on the equilibrium. While this question focuses on reaction rate, note that removing a reactant can also shift the equilibrium position of the reaction (Le Chatelier's Principle), but this is separate from the immediate rate change.

Conclude that removing some H₂(g) decreases the frequency of effective collisions between H₂ and NO molecules, leading to a slower reaction rate.

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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 a chemical reaction, if a reactant is removed, the equilibrium will shift to produce more of that reactant, thereby increasing the rate of the reaction until a new equilibrium is established.

Reaction Rate

The reaction rate refers to the speed at which reactants are converted into products in a chemical reaction. It can be influenced by various factors, including concentration, temperature, and the presence of catalysts. In this case, removing H₂(g) decreases its concentration, which can slow down the reaction rate as there are fewer reactant molecules available to collide and react.

Equilibrium Constant (K)

The equilibrium constant (K) is a numerical value that expresses the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. Changes in concentration, such as removing H₂(g), can affect the position of equilibrium but do not change the value of K. Understanding K helps predict how the system will respond to changes in concentration.

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