Interpretation:
To predict the exothermic and endothermic reactions should be identified given set of reaction and its images with different temperature.
Concept Introduction:
Equilibrium constant: Concentration of the products to the respective molar concentration of reactants it is called equilibrium constant. If the K value is less than one the reaction will move to the left side and the K values is higher (or) greater than one the reaction will move to the right side of reaction.
Free energy: The change in the standard energy of the system that occurs during a reaction is therefore equal to the change in the enthalpy
Exothermic and endothermic reaction: This type of chemical reaction release energy by light or heat. This type of
Want to see the full answer?
Check out a sample textbook solutionChapter 15 Solutions
CHEMISTRY: ATOMS FIRST ALEKS CODE
- Complete the changes in concentrations (or pressure, if requested) for each of the following reactions‘ (a) 2H2(g)+O2(g)2H2O(g) + 2x 1.50M (b) CS2(g)+4H2(g)CH4(g)+2H2S(g) x 0.020 M (c) Change in pressure: H2(g)+CI2(g)2HCI(g)x 1.50 atm (d) Change in pressure: 2NH3(g)+2O2(g)N2O(g)+3H2O(g) x = 60.6 torr (e) NH4HS(s)NH3+H2S(g) x 9.8106M (f) Change in pressure: Fe(s)+5CO(g)Fe(CO)5(g) x 0.012 atmarrow_forwardIs a system at equilibrium if the rate constants of the forward and reverse reactions are equal?arrow_forwardConsider the reaction N2O4(g)2NO2(g). Draw a graph illustrating the changes of concentrations of N2O4 and NO2 as equilibrium is approached. Describe how the rates of the forward and reverse reactions change as the mixture approaches dynamic equilibrium. Why is this called a dynamic equilibrium?arrow_forward
- Complete the changes in concentrations (or pressure, if requested) for each of the following reactions. (a) 2SO3(g)2SO2+O2(g) + x 0.125 M (b) 4NH3(g)+3O2(g)2N2(g)+6H2O(g) 3x 0.24 M (c) Change in pressure: 2CH4(g)C2H2(g)+3H2(g) x 25 torr (d) Change in pressure: CH4(g)+H2O(g)CO(g)+3H2(g) x 5 atm (e) CH4CI(s)NH3(g)+HCI(g) x 1.03104 M (e) Change in pressure: Ni(s)+4CO(g)Ni(CO)4(g) 4x 0.40 atmarrow_forwardFor the reaction A2 + 2B 2AB, diagram I depicts an initial reaction mixture, where A2 molecules are red and B atoms are green. Which of the diagrams II through IV is a possible equilibrium state for the reaction system? There may be more than one correct answer.arrow_forwardFor the reaction A2 + B2 2AB, diagram I depicts an initial reaction mixture, where A2 molecules are red and B2 molecules are green. Which of the diagrams II through IV is a possible equilibrium state for the reaction system? There may be more than one correct answer.arrow_forward
- Suggest four ways in which the concentration of hydrazine, N2H4, could be increased in an equilibrium described by the following equation: N2(g)+2H2(g)N2H4(g)H=95kJarrow_forward. Plants synthesize the sugar dextrose according to the following reaction by absorbing radiant energy from the sun (photosynthesis). 6CO2(g)+6H2O(g)C6H12O6(g)+6O2(g)Will an increase in temperature tend to favor or discourage the production of C6H12O6(s)?arrow_forward. 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?arrow_forward
- . In your own words, paraphrase Le Châtelier’s principle. Give an example (including a balanced chemical equation) of how each of the following changes can affect the position of equilibrium in favor of additional products for a system: the concentration of one of the reactants is increased: one of the products is selectively removed from the system: the reaction system is compressed to a smaller volume: the temperature is increased for an endothermic reaction: the temperature is decreased for an exothermic process.arrow_forwardSuppose 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?arrow_forwardAmmonium hydrogen sulfide. NH4HS, is unstable at room temperature and decomposes: NH4HS(s)NH3(g)+H2S(g) You have placed some solid ammonium hydrogen sulfide in a closed flask. Which of the following would produce less hydrogen sulfide, H2S, which is a poisonous gas? a Removing some NH3 from the flask b Adding some NH3 to the flask c Removing some of the NH4HS d Increasing the pressure in the flask by adding helium gasarrow_forward
- General, Organic, and Biological ChemistryChemistryISBN:9781285853918Author:H. Stephen StokerPublisher:Cengage LearningIntroduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage LearningIntroductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
- Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStaxGeneral Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning