Physical Chemistry
2nd Edition
ISBN: 9781133958437
Author: Ball, David W. (david Warren), BAER, Tomas
Publisher: Wadsworth Cengage Learning,
expand_more
expand_more
format_list_bulleted
Textbook Question
Chapter 5, Problem 5.38E
At what pressure does
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
calculate the Gibbs free energy of formation of BiF5 at 298 K.
Is the formation of BiF5 from the elements spontaneous?
Assuming that neither standard enthalpy changes of formations (∆Hof) nor standard molar entropies (So) depend upon temperature, estimate using the Table of Thermodynamic Data : (a) the standard Gibbs free energy change for the reaction that forms rhombic sulfur at 600 K, and (b) the temperature (in oC) at which reaction will stop formation of products:
2H2S(g) + SO2(g) → 3S(rhombic, s) + 2H2O(g)
Round off your answers to the nearest integer. Report the temperature in oC. and enter them with correct units:
(a)∆Gorxn =
(b) T =
(a) The equilibrium constant of the isomerization of cis-2-butene to trans-2-butene is 2.07 at
127.0 °C. Determine the standard molar Gibbs free energy, AGR º for the reaction.
(b) For C6o, the standard molar Gibbs free energy (AG, º) of formation from the elemental carbon
is 23.98 kJ/mol at 25.0 °C. Determine the equilibrium constant, Keq for the formation of C60.
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
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- Actually, the carbon in CO2(g) is thermodynamically unstable with respect to the carbon in calcium carbonate(limestone). Verify this by determining the standardGibbs free energy change for the reaction of lime,CaO(s), with CO2(g) to make CaCO3(s).arrow_forwardUse the appropriate tables to calculate H for (a) the reaction between copper(II) oxide and carbon monoxide to give copper metal and carbon dioxide. (b) the decomposition of one mole of methyl alcohol (CH3OH) to methane and oxygen gases.arrow_forwardIn the late eighteenth century Priestley prepared ammonia by reacting HNO3(g) with hydrogen gas. The thermodynamic equation for the reaction is HNO3(g)+4H2(g)NH3(g)+3H2O(g)H=637kJ (a) Calculate H when one mole of hydrogen gas reacts. (b) What is H when 10.00 g of NH3(g) are made to react with an excess of steam to form HN3(g) and H2 gases?arrow_forward
- Calcium carbide, CaC2, is manufactured by reducing lime with carbon at high temperature. (The carbide is used in turn to make acetylene, an industrially important organic chemical.) Is the reaction endothermic or exothermic?arrow_forwardWhich molecule, F2, Cl2, Br2, or I2, has the weakest chemical bond?arrow_forwardThe lead-acid storage battery is the oldest rechargeable battery in existence. It was invented in 1859 by French physician Gaston Plante and still retains application todaY, more than 150 years later. There are two reactions that take place during discharge of the lead-acid storage battery. In one step, sulfuric acid decomposes to form sulfur trioxide and water: H, SO,() – SO;(9) + H,O() AH-+113. kJ In another step, lead, lead(IV) oxide, and sulfur trioxide react to form lead(II) sulfate: Pb(s) – PbO,(s) - 2 S0, (g) → 2 PbSO,(s) AH= -775. J Calculate the net change in enthalpy for the formation of one mole of lead(II) sulfate from lead, lead(IV) oxide, and sulfuric acid from these reactions. Round your answer to the nearest kJ.arrow_forward
- Estimate the difference between AH reaction and AU reaction (in kJ/mol) for the reaction: N₂H4(l) + 2H₂O₂(1)→N₂(g) + 4H2₂O(l) at 298 Karrow_forwardWhat pressure is required to achieve a CO2 concentration of 0.0690 mol L−1 at 20∘C?arrow_forward(28) The standard Gibbs free energy associated with the following reaction is -91.2 kJ: HCI (g) + NH3 (g) → NH,CI (s) What will be the value of AG,nn if the reaction takes place at 42.2°C, the partial pressure of HCI (g) is 0.788 atm and the partial pressure of NH3 (g) is 0.284 atm? (A) (B) -95.1 kl -90.7 kl (C) (D) (E) 3.93 kJ noltemol or ni lu bluos noinsou -79.5 kJ -87.3 kJarrow_forward
- magine the pressure of oxygen in the room you are in currently has a pressure of 0.250 atmospheres and the room is completely sealed (closed off from the surroundings). What do you expect to have a bigger effect on the PO2, increasing the temperature by 10°C or decreasing the size of the room by exactly half? You can assume the temperature of the room starts atapproximately 25°C (298 K).arrow_forward1)State the First Law of Thermodynamics. 2)Fluorine (F2) and iodine (I2) are both Group 17 elements. Explain with reference to intermolecular forces, why fluorine is a gas and iodine is a solid at room temperature. 4)When 30 g of ammonium nitrate, (NH4NO3) was stirred into 10 cm3 of water, the temperature fell from 21 oC to 15 oC. 5)Calculate the total amount of energy (E) released in this experiment. Ignore the heat capacity of ammonium nitrate. Take the specific heat capacity of the water as 4.18 J g-1 ºC-1. Density of water is 1.00 gcm-3. 6)This amount of energy [answer to part (i)] was produced by 30 g of ammonium nitrate. Calculate the energy change per mole of ammonium nitrate. Include the correct sign for…arrow_forwardThe calibration of a calorimeter is done by using 13.00mL of 0.104M NaOH and 11.29mL of 0.125M HCl (deltaH=-55.85 kJ/mol). An increase in temperature, 4.6 degC is recorded. In the similar calorimeter, 7.58mL of 0.151M of a compound X(OH)3 reacts with 9.60mL of 0.125M HCl. The temperature changed from 25.9degC to 23.4degC. Determine the heat capacity of calorimeter, ad the enthalpy of the reaction of X(OH)3 and HCl.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningPrinciples of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Principles of Modern Chemistry
Chemistry
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:Cengage Learning
Chemical Equilibria and Reaction Quotients; Author: Professor Dave Explains;https://www.youtube.com/watch?v=1GiZzCzmO5Q;License: Standard YouTube License, CC-BY