Table of contents

1. The Chemical World9m
- The Scientific Method
  9m
2. Measurement and Problem Solving2h 19m
3. Matter and Energy2h 15m
4. Atoms and Elements2h 33m
5. Molecules and Compounds1h 50m
6. Chemical Composition1h 23m
7. Chemical Reactions1h 43m
8. Quantities in Chemical Reactions1h 8m
9. Electrons in Atoms and the Periodic Table2h 32m
10. Chemical Bonding2h 10m
11 Gases2h 7m
12. Liquids, Solids, and Intermolecular Forces1h 11m
13. Solutions3h 1m
14. Acids and Bases2h 14m
15. Chemical Equilibrium1h 27m
16. Oxidation and Reduction1h 33m
17. Radioactivity and Nuclear Chemistry53m

15. Chemical Equilibrium

Le Chatelier's Principle

Introduction to Chemistry

15. Chemical Equilibrium

Le Chatelier's Principle

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Multiple Choice

Which direction will the following reaction (in a 10.0 L flask) proceed if a catalyst is added to the system?
CaCO₃ (s) ⇌ CaO (s) + CO₂ (g) K_p = 3.2 x 10^-28

To the right.

To the left.

The equilibrium position will not change but the rate will increase.

The equilibrium position will not change but the concentrations of everything will increase.

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Verified step by step guidance

Identify the role of a catalyst in a chemical reaction. A catalyst speeds up the rate of a reaction without being consumed, but it does not affect the equilibrium position of the reaction.

Understand the equilibrium constant (Kp) provided. The equilibrium constant is a measure of the ratio of the concentrations of products to reactants at equilibrium. A very small Kp value, like 3.2 x 10^-28, indicates that the reaction heavily favors the reactants at equilibrium.

Recognize that the addition of a catalyst does not change the value of Kp or the equilibrium concentrations of the reactants and products. It only affects the rate at which equilibrium is reached.

Consider the physical states of the reactants and products. In this reaction, CaCO3 and CaO are solids, and CO2 is a gas. The equilibrium expression for Kp only includes gases, so only the concentration of CO2 is relevant for Kp.

Conclude that adding a catalyst will increase the rate at which equilibrium is achieved, but it will not change the equilibrium position or the concentrations of the reactants and products at equilibrium. Therefore, the equilibrium position will not change, but the rate will increase.