The following reaction is exothermic: 3A(g) <---> B(g) + C(g) Gaseous argon is added to the equilibrium mixture without change in volume or temperature. Predict the effect of the possible stress mentioned directly above on the reaction mixture by selecting the correct phrase be O shift right to attain chemical equilibrium no shift to attain chemical equilibrium shift left to attain chemical equilibrium not enough information to answer question

The following reaction is exothermic: 3A(g) <---> B(g) + C(g) Gaseous argon is added to the equilibrium mixture without change in volume or temperature. Predict the effect of the possible stress mentioned directly above on the reaction mixture by selecting the correct phrase be O shift right to attain chemical equilibrium no shift to attain chemical equilibrium shift left to attain chemical equilibrium not enough information to answer question

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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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.
Hydrogen fluoride is produced by reacting hydrogen with fluorine according to the following equation H₂ (g) + F2 (g) → 2 HF (g) Please use the following information to answer the next question. A stress that would shift the equilibrium towards the products would be to O add HF(g) O remove H₂(g) O decrease the volume of the reaction vessel O decrease the temperature of the reaction vessel AH = -542.2 kJ
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
i See Periodic Table See Hin Increasing the concentration of a reactant shifts the position of chemical equilibrium towards formation of more products. What effect does adding a reactant have on the rates of the forward and reverse reactions? Choose one: O There is no effect on the forward and reverse reactions. For an equilibrium reaction, the forward and reverse rates are always equal. O Both the forward and reverse reactions speed up by the same amount. O The forward reaction speeds up immediately. As more product is made, the reverse reaction starts to speed up as the forward reaction starts to slow down until they are equal. O The forward reaction slows down initially. As the reaction proceeds, the reverse reaction slows down to meet the new forward reaction. O The forward reaction speeds up. Eventually, production of the product speeds up the reverse reaction rate to match the new forward rate. O It is impossible to say without more specific information.
QUESTION 25 Consider the following reversible reaction at equilibrium: 3 H2(g) + N2(g) → 2NH3(g) + heat Which of the following changes will shift the equilibrium towards the reactants (left side)? O Decreasing the temperature. O Increasing the amount of H2. O Adding a catalyst to the system. O Decreasing the volume of the system. O Increasing the amount of NH3.
Which of the following statements is FALSE: Group of answer choices The value of the equilibrium constant depends on the temperature Pure solids are not included in the equilibrium constant expression. At equilibrium, the reaction has stopped At equilibrium, the concentrations of all species are constant At equilibrium, the forward and reverse reactions are happening at the same rate
K values are often written and scientific notation. If a K value has a positive power of 10 does equilibrium favor the products or reactants.
Consider the following system at equilibrium: CH4(g) + 2H20(g) CO2(g) + 4H2(g) What change will cause the equilibrium to shift to form more CH4? Multiple Choice decrease (H2] increase (H20] decrease the volume of the reaction vessel increase (CH4] decrease [CO2] DELL
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 backwards toward equilibrium the reverse rate drops. As a reaction proceeds forward toward equilibrium the reverse rate rises. At equilibrium the speed of a reaction equals its rate constant. As a reaction proceeds backwards toward equilibrium the forward rate rises. At equilibrium the forward rate equals zero. X
MOving to anotrie question will save this response. Question 7 A state of dynamic equilibrium, Ag2CO3(s) +→ 2Ag*(aq) + CO32(aqg), exists in solutida. Which direction will the equilibrium shift if Ca(NO3)2(aq) is added to the system? O To the left. O To the right. O It will not shift left or right. A Moving to another question will save this response. MacBook Pro 80 888 FS F6 F7 FA esc F2 %23 2$ 8. 2 3 4. Q K A D 5
C(s) + H2O(g) (g) + H2(g) Fill in the table below showing how the change to the equilibrium will affect the indicated species when a new equilibrium position is established Change Quantity Effect Add H20(g) H2(g) Add C(s) CO(g) Decrease the volume C(s) Increase the volume H2(g) Add argon gas H20(g) Decrease the volume Total Pressure Increase the Temperature H2O(g) Increase the Temperature Ko