19. Chemical Thermodynamics
Gibbs Free Energy And Equilibrium
19. Chemical Thermodynamics
Gibbs Free Energy And Equilibrium - Video Tutorials & Practice Problems
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1
concept
∆Gº and K
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2
example
Gibbs Free Energy And Equilibrium Example
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3
Problem
ProblemFor reaction, Ag2CO3 (s) ⇌ Ag2O (s) + CO2 (g), the ∆Hº = 79.14 kJ/mol, ∆Sº = 167.2 J/K.
Determine the equilibrium constant at which the temperature is 365.1 K.
A
1.90 × 10−9
B
8.23 × 10−21
C
388.1
D
2.58 × 10−3
4
concept
∆G, ∆Gº and Q
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5
Problem
ProblemConsider a hypothetical reaction at 38 ºC, X2 (aq) + 2 Y (s) ⇌ 3 Z (aq), with a ∆G of −75.8 kJ.
Concentrations of reactants and products: [X2] = 1.4 M, [Y] = 0.34 M, [Z] = 2.6 M. Calculate Keq of this given reaction.
A
4.13 × 1015
B
2.67 × 1011
C
9.60 × 1012
D
6.67 × 1013
6
example
Gibbs Free Energy And Equilibrium Example
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PRACTICE PROBLEMS AND ACTIVITIES (48)
- Consider the sublimation of iodine at 25.0 °C : I2(s) ¡ I2( g) b. Find ΔG rxn at 25.0 °C under the following n...
- Consider the evaporation of methanol at 25.0 °C : CH3OH(l ) ¡ CH3OH( g) b. Find ΔG r at 25.0 °C under the fol...
- Formation constants for the ammonia and ethylenediamine complexes of nickel(II) indicate that Ni(en)32+ is muc...
- Spinach contains a lot of iron but is not a good source of dietary iron because nearly all the iron is tied up...
- Nitrogen reacts with fluorine to form nitrogen trifluoride: Calculate ∆G°, and determine whether the equilibr...
- Ammonium hydrogen sulfide, a stink bomb ingredient, decomposes to ammonia and hydrogen sulfide: Calculate the...
- Consider the reaction: CO2( g) + CCl4( g) ∆ 2 COCl2( g) Calculate ΔG for this reaction at 25 °C under the foll...
- Use data from Appendix IIB to calculate the equilibrium constants at 25 °C for each reaction. b. 2 H2S( g) ∆ 2...
- Use data from Appendix IIB to calculate the equilibrium constants at 25 °C for each reaction. a. 2 CO( g) + O2...
- Consider the reaction: I2( g) + Cl2( g) ∆ 2 ICl( g) K p = 81.9 at 25 °C Calculate ΔG rxn for the reaction at 2...
- Consider the reaction: I2( g) + Cl2( g) ∆ 2 ICl( g) K p = 81.9 at 25 °C Calculate ΔG rxn for the reaction at 2...
- Consider the reaction: I2( g) + Cl2( g) ∆ 2 ICl( g) K p = 81.9 at 25 °C Calculate ΔG rxn for the reaction at 2...
- Consider the reaction 2 NO21g2¡N2O41g2. (a) Using data from Appendix C, calculate ΔG° at 298 K. (b) Calculate ...
- Consider the reaction 3 CH41g2¡C3H81g2 + 2 H21g2. (b) Calculate ΔG at 298 K if the reaction mixture consists o...
- Using data from Appendix C, write the equilibrium-constant expression and calculate the value of the equilibri...
- Consider the reaction: 2 NO( g) + O2( g) ∆ 2 NO2( g) The following data show the equilibrium constant for this...
- Consider the decomposition of barium carbonate: BaCO31s2ΔBaO1s2 + CO21g2 Using data from Appendix C, calculate...
- Consider the decomposition of barium carbonate: BaCO31s2ΔBaO1s2 + CO21g2 Using data from Appendix C, calculate...
- Consider the reaction PbCO31s2ΔPbO1s2 + CO21g2 Using data in Appendix C, calculate the equilibrium pressure of...
- A reaction has an equilibrium constant of 8.5 * 103 at 298 K. At 755 K, the equilibrium constant is 0.65. Fin...
- The value of Ka for nitrous acid 1HNO22 at 25 °C is given in Appendix D. (c) What is the value of ΔG at equili...
- The value of Ka for nitrous acid 1HNO22 at 25 °C is given in Appendix D. (b) By using the value of Ka, calcula...
- The value of Ka for nitrous acid 1HNO22 at 25 °C is given in Appendix D. (d) What is the value of ΔG when 3H+4...
- Nitrogen dioxide, a pollutant in the atmosphere, can combine with water to form nitric acid. One of the possib...
- Consider this reaction occurring at 298 K: N2O( g) + NO2( g) ∆ 3 NO( g) b. If a reaction mixture contains only...
- Consider this reaction occurring at 298 K: BaCO3(s) ∆ BaO(s) + CO2( g) b. If BaCO3 is placed in an evacuated f...
- Living organisms use energy from the metabolism of food to create an energy-rich molecule called adenosine tri...
- Consider the following three reactions: (i) Ti1s2 + 2 Cl21g2¡TiCl41g2 (a) For each of the reactions, use data ...
- Using the data in Appendix C and given the pressures listed, calculate Kp and ΔG for each of the following rea...
- Dinitrogen tetroxide decomposes to nitrogen dioxide: N2O4( g) ¡ 2 NO2( g) ΔHrxn ° = 55.3 kJ At 298 K, a reac...
- The oxidation of glucose 1C6H12O62 in body tissue produces CO2 and H2O. In contrast, anaerobic decomposition, ...
- A metal salt with the formula MCl2 crystallizes from water to form a solid with the composition MCl2 # 6 H2O....
- The potassium-ion concentration in blood plasma is about 5.0 * 10-3 M, whereas the concentration in muscle-cel...
- Use the data in Appendix B to calculate ∆G for the decom-position of nitrosyl chloride at 25 °C when the parti...
- Consider the following equilibrium: N2O41g2Δ2 NO21g2 Thermodynamic data on these gases are given in Appendix C...
- The Haber process is the principal industrial route for converting nitrogen into ammonia: N21g2 + 3 H21g2 ¡ 2 ...
- The reaction SO21g2 + 2 H2S1g2Δ3 S1s2 + 2 H2O1g2 is the basis of a suggested method for removal of SO2 from po...
- Urea (NH2CONH2), an important nitrogen fertilizer, is produced industrially by the reaction Given that ∆G° =...
- Use the data in Appendix B to calculate the equilibrium pressure of CO2 in a closed 1 L vessel that contains e...
- Consider the Haber synthesis of gaseous NH3 (∆H°f = -46.1 kJ/mol; ∆G°f = -16.5 kJ/mol: (d) What are the equi...
- The normal boiling point of bromine is 58.8 °C, and the standard entropies of the liquid and vapor are S°[Br2(...
- A mixture of 14.0 g of N2 and 3.024 g of H2 in a 5.00 L container is heated to 400 °C. Use the data in Appendi...
- The lead storage battery uses the reaction (b) Calculate ∆G for this reaction on a cold winter's day (10 °F)...
- NaHCO3 ⇌ NaOH(s) + CO2(g) Calculate the value of the equilibrium constant.
- Calculate the equilibrium constant at 25°C for a reaction for which ∆G° = -4.22 kcal/mol.
- What is δg° for the following reaction at 25 °C? COBr2(g) ⇌ CO(g) + Br2(g) Kp = 4.11 × 104
- When two reactions are coupled in a cell, what determines if they will both proceed spontaneously?
- Br2(g) + Cl2(g) → BrCl(g) ΔG°f for brcl(g) is -1.0 kj/mol