A system at equilibrium has more of a reactant gas injected into the container. Which statement is more correct with respect to the reaction after the injection? A new equilibrium position is established with a new Keq value that is larger than the original Keq A new equilibrium position is established with the same Keq as the original system A new Keq now exists and must be experimentally determined A new equilibrium position is established with a new Keq value that is smaller than the original Keq

A system at equilibrium has more of a reactant gas injected into the container. Which statement is more correct with respect to the reaction after the injection? A new equilibrium position is established with a new Keq value that is larger than the original Keq A new equilibrium position is established with the same Keq as the original system A new Keq now exists and must be experimentally determined A new equilibrium position is established with a new Keq value that is smaller than the original Keq

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 12CR

See similar textbooks

Similar questions

Consider an equilibrium mixture of four chemicals (A. B. C. and D. all gases) reacting in a closed flask according to the following equation: A+BC+Da. You add more A to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is re-established? Justify your answer. h. You have the original set-up at equilibrium, and add more D to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is re-established? Justify your answer.
. 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 re-established by completing the table. Complete the table with the terms increase, decrease, or no change. N2 H2 NH3 Add N2(g) Remove H2(g) Add NH3(g) Add Ne(g) (constant V) Increase the temperature Decrease the volume (constant T) Add a catalyst
Write an equilibrium expression for each of the following gaseous reactions: a.3O22O3 b.COCl2CO+Cl2 c.CS2+4H2CH4+2H2S d.2SO2+O22SO3 e.CO+H2OCO2+H2
Tell what will happen to each equilibrium concentration in the following when the indicated stress is applied and a new equilibrium position is established. a. H+(aq)+HCO3(aq)H2O(l)+CO2(g); HCO3is added. b. CO2(g)+H2O(l)H2CO3(aq)+heat; CO2is removed. c. CO2(g)+H2O(l)H2CO3(aq)+heat; The system is cooled.
Tell what will happen to each equilibrium concentration in the following when the indicated stress is applied and a new equilibrium position is established. a. LiOH(s)+CO2(g)LiHCO3(s)+heat; CO2 is removed. b. 2NaHCO3(s)+heatNa2O(s)+2CO2(g)+H2O(g); The system is cooled. c. CaCO3(s)+heatCaO(s)+CO2(g); The system is cooled.
How does equilibrium represent the balancing of opposing processes? Give an example of an “equilibrium” encountered in everyday life, showing how the processes involved oppose each other.
When writing a chemical equation for a reaction that comes to equilibrium. how do we indicate symbolically that the reaction is reversible?
. Consider an equilibrium mixture consisting of H2O(g), CO(g). H2(g), and CO2(g) reacting in a closed vessel according to the equation H2O(g)+CO(g)H2(g)+CO2(g)a. You add more H2O to the flask. How does the new equilibrium concentration of each chemical compare to its origin al equilibrium concentration after equilibrium is re-established? Justify your answer. b. You add more H2to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is re-established? Justify your answer.
. For the reaction system C(s)+H2O(g)H2(g)+CO(g)which has already reached a state of equilibrium, predict the effect that each of the following changes will have on the position of the equilibrium. Tell whether the equilibrium will shift to the right, will shift to the left, or will not be affected. a. The pressure of hydrogen is increased by injecting an additional mole of hydrogen gas into the reaction vessel. b. Carbon monoxide gas is removed as it forms by use of a chemical absorbent or “scrubber.” c. An additional amount of solid carbon is added to the reaction vessel.