Which of the following occurs when reactants are removed from achemical reaction in solution or the gas phase at equilibrium? *O Product increases, so the equilibrium shifts to produce more products.O Reactant increases, so the equilibrium shifts to produce more products.O Reactants decreases, so the equilibrium shifts to produce more reactants.O Product decreases, so the equilibrium shifts to produce more reactants.The reaction [20 CO2 + 22 H:O → 2 Cz0H22 + 31 O:], in general terms, is:ReversibleO IrreversibleThe reaction [N:O: = 2 NO: ], in general terms, is: *ReversibleIrreversible

According to lechatliers principle when a system at equilibrium is subjected to a stress (change in…

Which of the following occurs when reactants are removed from a chemical reaction in solution or the gas phase at equilibrium? * Product increases, so the equilibrium shifts to produce more products. Reactant increases, so the equilibrium shifts to produce more products. Reactants decreases, so the equilibrium shifts to produce more reactants. Product decreases, so the equilibrium shifts to produce more reactants.

Which of the following occurs when reactants are removed from a chemical reaction in solution or the gas phase at equilibrium? * Product increases, so the equilibrium shifts to produce more products. Reactant increases, so the equilibrium shifts to produce more products. Reactants decreases, so the equilibrium shifts to produce more reactants. Product decreases, so the equilibrium shifts to produce more reactants.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 121QRT: When a mixture of hydrogen and bromine is maintained at normal atmospheric pressure and heated above...

See similar textbooks

Similar questions

. Explain what it means that a reaction has reached a state of chemical equilibrium. Explain why equilibrium is a dynamic state: Does a reaction really “stop” when the system reaches a state of equilibrium? Explain why, once a chemical system has reached equilibrium, the concentrations of all reactants remain constant with time. Why does this constancy of concentration not contradict our picture of equilibrium as being dynamic? What happens to the rates of the forward and reverse reactions as a system proceeds to equilibrium from a starting point where only reactants are present?
. 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
. What is the effect on the equilibrium position if an exothermic reaction is carried out at a higher temperature? Does the net amount of product increase or decrease? Does the value of the equilibrium constant change if the temperature is increased? If so, how does it change’?
Based on the diagrams, chemical reaction, and reaction conditions depicted in Problem 9-83, which of the diagrams represents the equilibrium mixture if the numerical value of the equilibrium constant is 9.0?
During an experiment with the Haber process, a researcher put 1 mol N2 and 1 mol H2 into a reaction vessel to observe the equilibrium formation of ammonia, NH3. N2(g)+3H2(g)2NH3(g) When these reactants come to equilibrium, assume that x mol H2 react. How many moles of ammonia form?
Hydrogen for use in ammonia production is produced by the reaction CH4(g)+H2O(g)750oCNicatalystCO(g)+3H2(g) What will happen to a reaction mixture at equilibrium if a. H2O(g) is removed? b. the temperature is increased (the reaction is endothermic)? c. an inert gas is added to a rigid reaction container? d. CO(g) is removed? e. the volume of the container is tripled?
. 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.
When writing a chemical equation for a reaction that comes to equilibrium. how do we indicate symbolically that the reaction is reversible?
Consider the reaction 2N2O(g) + O2(g) 4NO(g) Suppose the system is at equilibrium, and then an additional mole of N2O(g) is injected into the system at constant temperature. Once the reaction reestablishes equilibrium, has the amount of N2O increased or decreased from its original equilibrium amount? Explain. What happens to the value of the equilibrium constant with this change?
Suppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this constant tell you about the relative concentrations of products and reactants that will be present once equilibrium is reached? Is this reaction likely to be a good source of the products?
The value of the equilibrium constant, K, is dependent on which of the following? (There may be more than one answer.) a. the initial concentrations of the reactants b. the initial concentrations of the products c. the temperature of the system d. the nature of the reactants and products Explain.
When a mixture of hydrogen and bromine is maintained at normal atmospheric pressure and heated above 200. °C in a closed container, the hydrogen and bromine react to form hydrogen bromide and a gas-phase equilibrium is established. Write a balanced chemical equation for the equilibrium reaction. Use bond enthalpies from Table 6.2 ( Sec. 6-6b) to estimate the enthalpy change for the reaction. Based on your answers to parts (a) and (b), which is more important in determining the position of this equilibrium, the entropy effect or the energy effect? In which direction will the equilibrium shift as the temperature increases above 200. °C? Explain. Suppose that the pressure were increased to triple its initial value. In which direction would the equilibrium shift? Why is the equilibrium not established at room temperature?