Physical Chemistry
2nd Edition
ISBN: 9781133958437
Author: Ball, David W. (david Warren), BAER, Tomas
Publisher: Wadsworth Cengage Learning,
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Chapter 5, Problem 5.4E
Supersaturated solutions can be made in which more solute is dissolved in solution than would normally dissolve.
These solutions are inherently unstable, however. A seed crystal of calcium acetate,
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Chapter 5 Solutions
Physical Chemistry
Ch. 5 - 5.1. Can a battery that has a voltage be...Ch. 5 - 5.2. What is the difference between a static...Ch. 5 - Which system in each pair best represents...Ch. 5 -
5.4. Supersaturated solutions can be made in...Ch. 5 -
5.5. Following is a chemical reaction between...Ch. 5 - 5.6. The following is a reaction with its initial...Ch. 5 - The following is a reaction with initial amounts...Ch. 5 - 5.8. The hemoglobin in blood establishes an...Ch. 5 - Prob. 5.9ECh. 5 - 5.10. If and gases were contained in a system...
Ch. 5 - 5.11. Determine the numerical value of Q for the...Ch. 5 - 5.12. True or false: If all the partial pressures...Ch. 5 - For the reaction 2SO3(g)2SO2(g)+O2(g) when 2mol of...Ch. 5 - 5.14. Determine and for the following reaction at...Ch. 5 - 5.15. Consider the reaction
If the partial...Ch. 5 -
5.16. In atmospheric chemistry, the following...Ch. 5 - Prob. 5.17ECh. 5 - 5.18. Hydrogen cyanide can isomerize to hydrogen...Ch. 5 - 5.19. Assume that a reaction exists such that...Ch. 5 - Prob. 5.20ECh. 5 - 5.21. Show that if the coefficients of a balanced...Ch. 5 - 5.22. True or false: If for a gas-phase reaction,...Ch. 5 - 5.23. The balanced chemical reaction for the...Ch. 5 - The answers in exercise 5.23 should show that...Ch. 5 - At a high enough temperature, the equilibrium...Ch. 5 - Prob. 5.26ECh. 5 - 5.27. Nitrogen dioxide,, dimerizes easily to form...Ch. 5 - 5.28. Another nitrogen-oxygen reaction of some...Ch. 5 - Prob. 5.29ECh. 5 - Prob. 5.30ECh. 5 - Prob. 5.31ECh. 5 - 5.32. For the reaction
. (a) Using in Appendix...Ch. 5 - 5.33. Use the data in Appendix to calculate ...Ch. 5 - 5.34. The of diamond, a crystalline form of...Ch. 5 - 5.35. The densities of graphite and diamond are ...Ch. 5 - Buckminsterfullerene, C60, is a spherical molecule...Ch. 5 - Prob. 5.37ECh. 5 - At what pressure does H2O have an activity of...Ch. 5 - The bisulfate or hydrogen sulfate anion, HSO4, is...Ch. 5 - Prob. 5.40ECh. 5 - Write the equilibrium constant expression for each...Ch. 5 - Prob. 5.42ECh. 5 - For the given chemical equilibrium, these data are...Ch. 5 - Biological standard states include specifying a...Ch. 5 - a At 25.0C, Kw for the autoionization of water is...Ch. 5 - 5.46. For a reaction whose standard enthalpy...Ch. 5 - 5.47. For the reaction
and . Estimate for this...Ch. 5 - 5.48. The isotope exchange reaction
has an...Ch. 5 - 5.49. Consider the following equilibrium:
What...Ch. 5 - 5.50. For the equilibrium
Equilibrium partial...Ch. 5 - The decomposition of NaHCO3, used in kitchens to...Ch. 5 - 5.52. For the equilibrium
at,. In a flask, of...Ch. 5 - Prob. 5.53ECh. 5 - 5.54. For the reaction
The equilibrium...Ch. 5 - Prob. 5.55ECh. 5 - 5.56. Of the amino acids listed in Table , which...Ch. 5 - 5.57. Determine the concentration of the three...Ch. 5 - 5.58. The formation of zwitterionic glycine, ,...Ch. 5 - 5.59. Monosodium glutamate, or MSG, is the sodium...Ch. 5 - Prob. 5.60ECh. 5 - Consider the balanced chemical reaction...Ch. 5 - For the gas-phase reaction 2H2+O22H2O rxnG is...Ch. 5 - Prob. 5.63ECh. 5 - Prob. 5.64E
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- . 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_forwardWrite a chemical equation for an equilibrium system that would lead to the following expressions (ad) for K. (a) K=(PH2S)2 (PO2)3(PSO2)2 (PH2O)2 (b) K=(PF2)1/2 (PI2)1/2PIF (c) K=[ Cl ]2(Pcl2)[ Br ]2 (d) K=(PNO)2 (PH2O)4 [ Cu2+ ]3[ NO3 ]2 [ H+ ]8arrow_forwardExplain that equilibrium is dynamic, and that at equilibrium the forward and backward reaction rates are equal.arrow_forward
- 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.arrow_forwardWrite an equation for an equilibrium system that would lead to the following expressions (ac) for K. (a) K=(Pco)2 (PH2)5(PC2H6)(PH2O)2 (b) K=(PNH3)4 (PO2)5(PNO)4 (PH2O)6 (c) K=[ ClO3 ]2 [ Mn2+ ]2(Pcl2)[ MNO4 ]2 [ H+ ]4 ; liquid water is a productarrow_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_forward
- Write the equilibrium constant expression for each of the following reactions in terms of concentrations. (a) CO2(g) + C(s) 2 CO(g) (b) [Cu(NH3)4)2+(aq) Cu2+(aq) + 4 NH3(aq) (c) CH3CO2H(aq) + H2O() CH3CO2(aq) + H3O+(aq)arrow_forwardBecause calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go a step further and examine the equilibrium between carbonate ion and CaCOj. The reaction is Ca2+(aq) + COj2_(aq) ** CaCO,(s) The equilibrium constant for this reaction is 2.1 X 10*. If the initial calcium ion concentration is 0.02 AI and the carbonate concentration is 0.03 AI, what are the equilibrium concentrations of the ions? A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H2COj(aq) H+(aq) + HCO}‘(aq) K = 4.4 X 10"7 She starts with 0.1000 AI carbonic acid. What are the concentrations of all species at equilibrium?arrow_forwardDuring 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?arrow_forward
- 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?arrow_forwardFor the generalized chemical reaction A(g)+B(g)C(g)+D(g) determine whether the concentration of D in an equilibrium mixture will (1) increase, (2) decrease, or (3) not change when each of the following changes is effected. a. concentration of A is increased b. concentration of B is decreased c. concentration of C is increased d. concentration of C is decreasedarrow_forward. What does it mean to say that a state of chemical or physical equilibrium is dynamic?arrow_forward
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