Physical Chemistry
2nd Edition
ISBN: 9781133958437
Author: Ball, David W. (david Warren), BAER, Tomas
Publisher: Wadsworth Cengage Learning,
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Textbook Question
Chapter 5, Problem 5.10E
If
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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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- At the critical point for carbon dioxide, the substance is very far from being an ideal gas. Prove this statement by calculating the density of an ideal gas in g/cm3 at the conditions of the critical point and comparing it with the experimental value. Compute the experimental value from the fact that a mole of CO2 at its critical point occupies 94 cm3.arrow_forwardWhy is equation2.37 written interms of CV and Cp and not c-v and c-p ?arrow_forwardWhich of the following quantities can be taken to be independent of temperature? independent of pressure? (a) H for a reaction (b) S for a reaction (c) G for a reaction (d) S for a substancearrow_forward
- In the equation w = P V, why is there a negative sign?arrow_forwardA sample of nitrogen initially at T = 25 oC and p = 4.0 atm triples its initial volume. What will be its final temperature and pressure if it expands reversibly adiabatically?arrow_forwardIt is desired to market O2 in small cylinders having volumes of 15L and each containing 2 kg of O2. If the cylinders may be subjected to a maximum temperature of 500C, calculate the pressure, for which they may be designed, assume the applicability of the ideal gas law.arrow_forward
- A sample of air was compressed to a volume of 31.4 L. The temperature was 298 K and the pressure was 3.75 bar. How many moles of gas were in the sample? If the sample had been collected from air at p = 1.00 bar, T = 298 K, what was the original volume of the gas?n = --------- molV = ---------- Larrow_forwardQ#3 If the equation of state for a gas is described by the following equation: P.(V- b) =RT, where b=1200 cm3/mol Determine the ∆Ht when 5 moles of this gas go from State 1 (25°C, 10 bar) to State 2 (125°C, 20 bar). Assume CPig /R = 4arrow_forward2.00-mol of a monatomic ideal gas goes from State A to State D via the path A→B→C→D: State A PA=13.5atm, VA=11.50L State B PB=13.5atm, VB=7.00L State C PC=25.0atm, VC=7.00L State D PD=25.0atm, VD=25.00L Assume that the external pressure is constant during each step and equals the final pressure of the gas for that step. Calculate q for this process. Calculate w for this process. Calculate ΔE for this process Calculate ΔH for this process.arrow_forward
- Two guys where I grew up once threw a 25 kg chunk of sodium into the Eno River. When it hit the water, it exploded and shot back up into the air, over and over again for a few miles. Assuming that the pressure was 1 bar and 30 °C, how much work was done by the expanding gasthat was created by the reaction of sodium and water?arrow_forwardPlease solve using the equations: dCp/dt=-k(Cp) t1/2= 0.693/k Cp=C0e^-k(t)arrow_forward
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