Table of contents

1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 38m
5. BONUS: Mathematical Operations and Functions48m
6. Chemical Quantities & Aqueous Reactions3h 53m
7. Gases3h 49m
8. Thermochemistry2h 37m
9. Quantum Mechanics2h 58m
10. Periodic Properties of the Elements3h 9m
11. Bonding & Molecular Structure3h 29m
12. Molecular Shapes & Valence Bond Theory1h 57m
13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
20. Electrochemistry2h 42m
21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

6. Chemical Quantities & Aqueous Reactions

Redox Reactions

General Chemistry

6. Chemical Quantities & Aqueous Reactions

Redox Reactions

Previous problemNext problem

Struggling with General Chemistry?

Join thousands of students who trust us to help them ace their exams!Watch the first video

Multiple Choice

In a chemical equilibrium involving the reaction Q ⇌ S, which direction will the reaction favor if both Q and S are present in high concentrations?

The reaction will favor the formation of Q.

The reaction will favor the formation of S.

The reaction will favor the formation of both Q and S equally.

The reaction will remain at equilibrium with no net change.

Previous problemNext problem

Verified step by step guidance

Identify the concept of chemical equilibrium: In a chemical equilibrium, the rate of the forward reaction equals the rate of the reverse reaction, resulting in no net change in the concentrations of reactants and products over time.

Understand the role of concentration in equilibrium: According to Le Chatelier's Principle, if a system at equilibrium is disturbed by changing the concentration of reactants or products, the system will adjust to counteract the disturbance and restore a new equilibrium.

Analyze the given scenario: Both Q and S are present in high concentrations. This implies that the system is already at equilibrium or close to it, as both reactants and products are available in significant amounts.

Consider the effect of high concentrations: High concentrations of both Q and S suggest that the reaction has reached a state where the forward and reverse reactions are occurring at the same rate, maintaining equilibrium.

Conclude the direction of the reaction: Since both Q and S are present in high concentrations and the system is at equilibrium, there will be no net change in the concentrations of Q and S, meaning the reaction will remain at equilibrium.