Consider the exothermic reaction:
a. decrease
b. increase
c. decrease
d. increase temperature
e. decrease temperature
f. Increase pressure
(a)
Interpretation:
The effect of the decrease in the concentration of HI to the direction of equilibrium should be explained.
Concept Introduction:
The net concentrations of the reactants and products do not change at equilibrium, they are used to define an expression, the equilibrium constant (K) which has a characteristic value
For a reaction at a given temperature,
Le Chatelier's principle is a general rule used to explain the effect of a change in reaction conditions on equilibrium.
Le Chatelier's principle states:
If a chemical system at equilibrium is disturbed, equilibrium will shift in the direction to counteract the change.
Answer to Problem 70P
Equilibrium favor shift to right.
Explanation of Solution
Given information:
Reactants and products are in equilibrium. With decrease in the HI concentration, equilibrium is disturbed. Then rate of the forward reaction increases.
Equilibrium favors shift to right.
(b)
Interpretation:
The effect of the increase in the concentration of H2 to the direction of equilibrium should be explained.
Concept Introduction:
The net concentrations of the reactants and products do not change at equilibrium. They are used to define an expression and the equilibrium constant (K) which has a characteristic value.
For a reaction at a given temperature,
Le Chatelier's principle is a general rule used to explain the effect of a change in reaction conditions on equilibrium.
Le Chatelier's principle states:
If a chemical system at equilibrium is disturbed, equilibrium will shift in the direction to counteract the change.
Answer to Problem 70P
Equilibrium favors shift to right.
Explanation of Solution
Given information:
Reactants and products are in equilibrium. With an increase in H2 concentration, equilibrium is disturbed. Then rate of the forward reaction increases.
Equilibrium favors shift to right.
(c)
Interpretation:
The effect of the decrease in the concentration of I2 to the direction of equilibrium should be explained.
Concept Introduction:
The net concentrations of the reactants and products do not change at equilibrium. They are used to define an expression and the equilibrium constant (K) which has a characteristic value.
For a reaction at a given temperature,
Le Chatelier's principle is a general rule used to explain the effect of a change in reaction conditions on equilibrium.
Le Chatelier's principle states:
If a chemical system at equilibrium is disturbed, equilibrium will shift in the direction to counteract the change.
Answer to Problem 70P
Equilibrium favors shift to left.
Explanation of Solution
Given information:
Reactants and products are in equilibrium. With decrease of I2 concentration, equilibrium is disturbed. Then rate of the reverse reaction increases.
Equilibrium favors shift to the left.
(d)
Interpretation:
The effect of the increase in temperature to the direction of equilibrium should be explained.
Concept Introduction:
The net concentrations of the reactants and products do not change at equilibrium. They are used to define an expression and the equilibrium constant (K) which has a characteristic value.
For a reaction at a given temperature,
Le Chatelier's principle is a general rule used to explain the effect of a change in reaction conditions on equilibrium.
Le Chatelier's principle states:
If a chemical system at equilibrium is disturbed, equilibrium will shift in the direction to counteract the change.
Answer to Problem 70P
Equilibrium favors shift to left.
Explanation of Solution
Given information:
Reactants and products are in equilibrium. This is exothermic reaction.
Exothermic reaction release energy to drive the reaction.
With increase of temperature, equilibrium is disturbed. Then rate of the reverse reaction increases.
Equilibrium favor shift to left.
(e)
Interpretation:
The effect of the decrease in the temperature to the direction of equilibrium should be explained.
Concept Introduction:
The net concentrations of the reactants and products do not change at equilibrium. They are used to define an expression and the equilibrium constant (K) which has a characteristic value.
For a reaction at a given temperature,
Le Chatelier's principle is a general rule used to explain the effect of a change in reaction conditions on equilibrium.
Le Chatelier's principle states:
If a chemical system at equilibrium is disturbed, equilibrium will shift in the direction to counteract the change.
Answer to Problem 70P
Equilibrium favors shift to right.
Explanation of Solution
Given information:
Reactants and products are in equilibrium. This is exothermic reaction.
Exothermic reaction release energy to drive the reaction.
With decrease of temperature, equilibrium is disturbed.
Equilibrium favor shift to right.
(f)
Interpretation:
The effect of the increase of pressure to the direction of equilibrium should be explained.
Concept Introduction:
The net concentrations of the reactants and products do not change at equilibrium. They are used to define an expression and the equilibrium constant (K) which has a characteristic value.
For a reaction at a given temperature,
Le Chatelier's principle is a general rule used to explain the effect of a change in reaction conditions on equilibrium.
Le Chatelier's principle states:
If a chemical system at equilibrium is disturbed, equilibrium will shift in the direction to counteract the change.
Answer to Problem 70P
Equilibrium does not change.
Explanation of Solution
Given information:
Reactants and products are in equilibrium. Both reactant and products are gaseous molecules.
Therefore, with the increase of the pressure the equilibrium will shift towards the side of the reaction with fewer gas molecules.
In here, both sides have the same number of gas molecules. Therefore, equilibrium not changes.
Want to see more full solutions like this?
Chapter 6 Solutions
GENERAL,ORGANIC, & BIOLOGICAL CHEM-ACCES
Additional Science Textbook Solutions
Basic Chemistry (5th Edition)
Chemistry
General Chemistry: Principles and Modern Applications (11th Edition)
Principles of Chemistry: A Molecular Approach (3rd Edition)
Organic Chemistry (9th Edition)
- . Consider the reaction 2CO(g)+O2(g)2CO2(g)Suppose the system is already at equilibrium, and then an additional mole of CO2(g) is injected into the system at constant temperature. Does the amount of O2(g) in the system increase or decrease? Does the value of K for the reaction change?arrow_forwardConsider the system 4 NH3(g) + 3 O2(g) ⇌ 2 N2(g) + 6 H20(ℓ) ΔrH° = −1530.4 kJ/mol How will the amount of ammonia at equilibrium be affected by removing O2(g) without changing the total gas volume? adding N2(g) without changing the total gas volume? adding water without changing the total gas volume? expanding the container? increasing the temperature? Which of these changes (i to v) increases the value of K? Which decreases it?arrow_forwardHydrogenation, the addition of hydrogen to an organic compound, is an industrially important reaction. Calculate rH, rS, and rG for the hydrogenation of octene, C8H16, to give octane, C8H19 at 25 C. Is the reaction product- or reactant-favored at equilibrium? C8H16(g) + H2(g) C8H18(g) Along with data in Appendix L, the following information is needed for this calculation.arrow_forward
- The following equilibrium is established in a closed container: C(s)+O2(g)CO2(g)H=393kJmol1 How does the equilibrium shift in response to each of the following stresses? (a) The quantity of solid carbon is increased. (b) A small quantity of water is added, and CO2 dissolves in it. (c) The system is cooled. (d) The volume of the container is increased.arrow_forward. 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.arrow_forwardWater gas, a mixture of H2 and CO, is an important industrial fuel produced by the reaction of steam with red hot coke, essentially pure carbon. (a) Write the expression for the equilibrium constant for the reversible reaction C(s)+H2O(g)CO(g)+H2(g)H=131.30kJ (b) What will happen to the concentration of each reactant and product at equilibrium if more C is added? (c) What will happen to the concentration of each reactant and product at equilibrium if H2O is removed? (d) What will happen to the concentration of each reactant and product at equilibrium if CO is added? (e) What will happen to the concentration of each reactant and product at equilibrium if the temperature of the system is increased?arrow_forward
- 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?arrow_forwardExplain why an equilibrium between Br2(l) and Br2(g) would not be established if the container were not a closed vessel shown in Figure 13.5.arrow_forwardKp for the following reaction is 0.16 at 25 C: 2 NOBr(g) 2 NO(g) + Br2(g) The enthalpy change for the reaction at standard conditions is + 16.3 kJ/mol-rxn. Predict the effect of the following changes on the position of the equilibrium; that is, state which way the equilibrium will shift (left, right, or no change) when each of the following changes is made. (a) adding more Br2(g) (b) removing some NOBr(g) (c) decreasing the temperature (d) increasing the container volumearrow_forward
- The formation of ammonia from its elements is an important industrial process. 3 H2(g) + N2(g) 2 NH3(g) 1. Does the reaction shift to the right or to the left, or does it remain unchanged, when extra H2 is added? (a) shift left (b) shift right (c)unchangedarrow_forwardPhosphorus pentachloride decomposes at elevated temperatures. PCl5(g) PCl3(g) + Cl2(g) An equilibrium mixture at some temperature consists of 3.120 g of PCl5, 3.845 g of PCl3, and 1.787 g of Cl2 in a 10.0-L flask. If you add 1.418 g of Cl2, how will the equilibrium be affected? What will the concentrations of PCl5, PCl3, and Cl2 be when equilibrium is reestablished?arrow_forwardConsider the decomposition of CaCO3(s) into CaO(s) and Co2(g). What is the equilibrium partial pressure of CO2 at room temperature?arrow_forward
- Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
- Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning