equilibrium ### Understanding Equilibrium Constant in Endothermic Reactions#### Question:As the temperature increases for an endothermic reaction, what happens to the equilibrium constant?#### Answer Choices:- **A) stays the same**- **B) increases**- **C) decreases**- **D) increases only if ΔS is negative**- **E) decreases only if ΔS is positive**For endothermic reactions, the equilibrium constant increases with an increase in temperature. This is due to the fact that increasing temperature favors the forward reaction, which absorbs heat. This follows Le Chatelier's principle, which states that the system will adjust to counteract the change (in this case, the temperature increase).To understand deeper, consider the Van't Hoff equation which shows the relationship between the equilibrium constant (K) and temperature (T):\[ \ln K = -\frac{\Delta H}{RT} + \frac{\Delta S}{R} \]Where:- \( \Delta H \) is the enthalpy change (positive for endothermic reactions).- \( R \) is the universal gas constant.- \( \Delta S \) is the entropy change.For an endothermic reaction (\(\Delta H > 0\)), an increase in \( T \) will increase \( K \) because \(\Delta H / RT\) decreases with increasing \( T \), leading to a larger value of \( K \). This aligns with option **B) increases**.

According to Le Chatelier’s principle, “When a system experiences any disturbance in the equilibrium…

Answered: equilibrium

Science

Chemistry

equilibrium

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...

See similar textbooks

Similar questions

How would adding a catalyst change shift of the equilibrium?
Decide whether each of the following statements is true or false. If false, change the wording of the statement to make it true. a) The magnitude of the equilibrium constant is always independent of temperature. b) When two chemical equations are added to give a net equation, the equilibrium constant for the net equation is the product of the equilibrium constants of the summed equations. c) The equilibrium constant for a reaction has the same value as K for the reverse reaction. d) Only the concentration of CO2 appears in the equilibrium expression for the reaction: CaCO3 (s) ↔ CaO (s) + CO2 (g). e) For the reaction CaCO3 (s) ↔ CaO (s) + CO2 (g), the value of K is numerically the same whether the amount of CO2 is expressed as molarity or as gas pressure.
The addition of a catalyst will change the composition of the equilibrium mixture. True False
In general, for a system at equilibrium, indicate the direction the equilibrium will shift for the following change. The concentration of one or more of the reactants is increased.
QUESTION 4 Adding a catalyst to an equilibrium system will: produce more products at equilibrium. produce more reactants at equilibrium. not change the amount of reactants or products at equilibrium.
Select the statement that is true about equilibrium reactions. large value for K (K >> 1) indicates the reaction lies to the right and favors products. K can be a negative value The rate of the reaction forward is equal to the rate of reaction in reverse. O The equilibrium constant is the ratio of the concentrations of the reactants to concentrations of products
An increase in product concentration drives the reaction towards more reactants. True O False
Record your two digit answer. Use the following information to answer the next 4 questions. An equilibrium system was established in a 1.00 L flask at a certain temperature as represented by the following equation ICI(g) + Cl₂(g) ICI,(g) + energy brown yellow-green bright yellow At equilibrium the flask contained 0.0571 mol of ICI(g), 1.07 mol of Cl₂(g), 1.87 mol of ICl3(g) The value of the equilibrium constant for this system is 30.6 Record your 3-digit answer Under these conditions, the equilibrium system in Question 20 favours the forward the reverse neither reaction. ?