### Chemical Equilibrium---#### Question:An increase in product concentration drives the reaction towards more reactants.- ○ **True**- ○ **False**---This is a simple multiple-choice question designed to test your understanding of Le Chatelier’s Principle in chemical equilibrium. The principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change. For example, if the concentration of reactants or products is changed, the equilibrium will shift to balance the effect of the change:1. **Increase in product concentration**: According to Le Chatelier’s Principle, the system will respond by shifting the equilibrium towards the reactants to decrease the product concentration.2. **Decrease in product concentration**: The equilibrium will shift towards producing more of the product to restore balance.In this context, the correct answer to the question is **True**.---##### Visual Aids Explanation:This section does not contain any graphs or diagrams; if it did, they would be explained in detail here to help illustrate the principle being tested. For example, a graph showing the change in concentration over time or a diagram of the equilibrium shift can be used for better comprehension. ---### Additional Information:- **Le Chatelier’s Principle** is crucial in understanding how chemical reactions respond to changes in concentration, temperature, or pressure.- This principle has practical applications in industrial processes, such as the Haber process for ammonia synthesis.For further reading, refer to the section on Chemical Equilibrium in your textbook.

If a chemical system is in equilibrium and if we try to to distrub the equilibrium, system try to…

Answered: ? An increase in product concentration…

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Chemistry

? An increase in product concentration drives the reaction towards more reactants. O True O False

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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2. Which of the following is most similar to a system at equilibrium? * O a shift change at an assembly plant involving two crews of 100 employees O a popcorn maker when the popcorn starts to pop the water in a pool when swimmers start to splash water out of the pool a burning candle salt concentrations in the oceans
Select all of the correct statements about equilibrium from the choices below.At equilibrium the rates of forward and reverse reactions are equal. As a reaction proceeds forward toward equilibrium the forward rate drops. At equilibrium all reactions stop. Reactants are transformed into products even at equilibrium. As a reaction proceeds forward toward equilibrium the reverse rate constant rises.As a reaction proceeds forward toward equilibrium the forward rate constant drops.
What happens to a system when products are added to a reaction vessel? O The amount of products increases. O The amount of reactants increases. O The amount of reactants decreases. O The system remains at equilibrium.
Select all of the correct statements about equilibrium from the choices below. At equilibrium the rates of forward and reverse reactions are equal. As a reaction proceeds forward toward equilibrium the reactant concentrations drop. Reactants are transformed into products even at equilibrium. As a reaction proceeds forward toward equilibrium the product concentrations rise. At equilibrium all reactions stop. As a reaction proceeds forward toward equilibrium the forward rate constant drops.
Which of the following is true for chemical equilibrium? I. Forward and reverse reaction rates are equalII. Equilibrium can be achieved from either directionIII. Reaction rates and therefore equilibrium is temperature-dependent. a I only b I and II only c II and III only d I, II and III
Consider the following reversible reaction at equilibrium: CO(g) + Cl2(g) COCI,(g). Use Le Chatelier's principle to predict the effect of adding some Cl2(g) to the equilibrium system? the concentration of CO(g) increases the concentration of COC12(g) decreases the equilibrium system shifts to the right to restore equilibrium the equilibrium system shifts to the left to restore equilibrium no effect
Le Chatelier’s principle allows scientists to predict shifts in equilibrium. If you increase the temperature on an exothermic reaction, which direction does equilibrium shift? Towards the reactants or towards the products?
Consider the exothermic reaction: C2H4(g) + Cl2(g) C2H,Cl,(g). What effect does each of the following changes have on the direction of equilibrium? d. decrease pressure a. increase [C2H4] b. decrease [Cl,] c. decrease [C2H¼CI,] e. increase temperature f. decrease temperature
According to Le Châtelier's principle, how will an increase in concentration of a reactant affect the equilibrium system? Shift it toward the products Shift it toward the reactants Shift it toward the side with higher total mole concentration or Shift it toward the side with lower total mole concentration
An abundance of product added to a system in equilibrium will push it towards O the reactant. O dynamic stasis. O dynamic equilibrium. the product. O O OO
Which statement best describes general equilibrium? O Equilibrium is reached when the reaction stops. O There is only one set of equilibrium concentrations that equals the Kc value. At equilibrium, the rate of the forward reaction is the same as the rate of the reverse reaction. At equilibrium, the total concentration of products equals the total concentration of reactants.
For questions 19-25. Consider the following exothermic reaction at equilibrium: N2(g) - 3H2(g) = 2NH3(g). Predict how the following changes affect the number of moles of each component of the system after equilibrium is reestablish. What will happen to N2? 24. Decrease the volume (constant T) * increase decrease no reaction