Search results
- What would be the effect of reducing the volume of a container in which the following system was at equilibrium? 2NO(g) + O2(g) ⇌ 2NO2(g) (a) decrease the rate (b) decrease K(c) decrease [NO2] (d) increase [NO2] (e) none of these.
- How would you increase the yield of product in the following reaction? SO2(g) + NO2(g) ---> SO3(g) + NO(g) ΔH o = −42 kJ. (a) increase temperature (b) decrease temperature (c) increase volume (d) decrease volume.
- What effect with the addition of a small amount of NaOH(s) have on the following system? CH3COOH(aq) + H2O(ℓ) ⇌ H3O(aq) + CH3COO¯(aq) (a) it changes the value of Kof CH3COOH.
- In the following closed system: CO(g) + 1⁄2O2 ⇌ CO2(g) ΔH° = −198 kJ. which one(s) of the following statements is (are) correct? I. Increasing the pressure would cause the quantity of CO2 to increase.
Jun 23, 2023 · Solution. According to Le Chatelier's principle, if pressure is increased, then the equilibrium shifts to the side with the fewer number of moles of gas. This particular reaction shows a total of 4 mol of gas as reactants and 2 mol of gas as products, so the reaction shifts toward the products side.
- The Concept of Equilibrium. Conceptual Problems. What is meant when a reaction is described as “having reached equilibrium”? What does this statement mean regarding the forward and reverse reaction rates?
- The Equilibrium Constant. Conceptual Problems. For an equilibrium reaction, what effect does reversing the reactants and products have on the value of the equilibrium constant?
- Interpreting & Working with Equilibrium Constants. Conceptual Problems. Describe how to determine the magnitude of the equilibrium constant for a reaction when not all concentrations of the substances are known.
- Heterogeneous Equilibria.
Jul 4, 2021 · Le Chatelier’s principle says that if a change is made to a system in dynamic equilibrium, the position of the equilibrium moves to counteract this change. The principle is used to predict changes to the position of equilibrium when there are changes in temperature, pressure or concentration.
Aug 26, 2023 · Reaction rates are affected primarily by concentrations, as described by the reaction’s rate law, and temperature, as described by the Arrhenius equation. Consequently, changes in concentration and temperature are the two stresses that can shift an equilibrium.
Practice Problems on Le Châtelier’s principle to understand the effect of changing concentration, volume, temperature, and pressure on equilibrium.
People also ask
Why does the equilibrium shift left in a reverse reaction?
Which two stresses can shift an equilibrium system?
Why does equilibria shift toward reactants?
How can chemical equilibria be shifted?
What happens if an equilibrium system is stressed?
How can we distinguish between a system that has reached equilibrium?
Solution. According to Le Chatelier’s principle, if pressure is increased, then the equilibrium shifts to the side with the fewer number of moles of gas. This particular reaction shows a total of 4 mol of gas as reactants and 2 mol of gas as products, so the reaction shifts toward the products side. Test Yourself.
