The AG for the reaction H2(g) + I2(g) = 2HI(g) is 2.60 kJ/mol at 25°C. In one experiment, the initial pressures are PH, 3 3.92 atm %3D = 0.026 atm PHI = 0.46 atm Calculate AG for the reaction and predict the direction of the net reaction kJ/mol The net reaction proceeds from left to right The reaction proceeds from right to left

The AG for the reaction H2(g) + I2(g) = 2HI(g) is 2.60 kJ/mol at 25°C. In one experiment, the initial pressures are PH, 3 3.92 atm %3D = 0.026 atm PHI = 0.46 atm Calculate AG for the reaction and predict the direction of the net reaction kJ/mol The net reaction proceeds from left to right The reaction proceeds from right to left

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter16: Spontaneity, Entropy, And Free Energy

Section: Chapter Questions

Problem 101CWP

See similar textbooks

Similar questions

Acetic acid, CH3CO2H, can form a dimer, (CH3CO2H)2, in the gas phase.. 2CH3CO2H(g)(CH3CO2H)2(g) The dimer is held together by to hydrogen bonds with a total strength of 66.5 kJ per mole of dimer. At 25 C, the equilibrium constant for the dimerization is 1.3103 (pressure in atm). What is ?S for the reaction?
The equilibrium constant for a certain reaction decreases from 8.84 to 3.25 102 when the temperature increases from 25C to 75C. Estimate the temperature where K = 1.00 for this reaction. Estimate the value of S for this reaction. (Hint: Manipulate the equation in Exercise 79.)
For the decomposition of Ag2O: 2Ag2O(s)4Ag(s)+O2(g)(a) Obtain an expression for G as a function of temperature. Prepare a table of G values at 100 K intervals between 100 K and 500 K. b) Calculate the temperature at which G =0.
Predict the temperature at which the reaction in Exercise 17.67 comes to equilibrium. Consider the equation G = H TS. At some value of T, G equals zero and the reaction is at equilibrium. Set G = 0, substitute for H and S (assuming that they do not vary much with temperature) and solve for T. CH3CHO(l)+52O2(g)2CO2(g)+2H2O(l)
Monochloroethane (C2H5Cl) can be produced by the direct reaction of ethane gas (C2H6) with chlorine gas or by the reaction of ethylene gas (C2H4) with hydrogen chloride gas. The second reaction gives almost a 100% yield of pure C2H5Cl at a rapid rate without catalysis. The first method requires light as an energy source or the reaction would not occur. Yet G for the first reaction is considerably more negative than G for the second reaction. Explain how this can be so.
Consider the reaction H2(g)+Br2(g)2HBr(g) where H = 103.8 kJ/mol. In a particular experiment, equal moles of H2(g) at 1.00 atm and Br2(g) at 1.00 atm were mixed in a 1.00-L flask at 25C and allowed to reach equilibrium. Then the molecules of H2 at equilibrium were counted using a very sensitive technique, and 1.10 1013 molecules were found. For this reaction, calculate the values of K, G, and S.
Describe how you would expect the spontaneity (G) for each of the following reactions to behave with a change of temperature. a Phosgene, COCl2, the starting material for the preparation of polyurethane plastics, decomposes as follows: COCl2(g)CO(g)+Cl2(g) b Chlorine is added to ethylene to produce dichloroethane, a solvent: Cl2(g)+C2H4(g)C2H4Cl2(l)
If wet silver carbonate is dried in a stream of hot air. the air must have a certain concentration level of carbon dioxide to prevent silver carbonate from decomposing by the reaction Ag2CO3(s)Ag2O(s)+CO2(g) H for this reaction is 79.14 kJ/mol in the temperature range of 25 to 125C. Given that the partial pressure of carbon dioxide in equilibrium with pure solid silver carbonate is 6.23 103 torr at 25C, calculate the partial pressure of CO2 necessary to prevent decomposition ofAg2CO3 at 110C. (Hint: Manipulate the equation in Exercise 79.)
Old-fashioned smelling salts consist of ammonium carbonate, (NH4)2CO3. The reaction for the decomposition of ammonium carbonate (NH4)2CO3(s)2NH3(g)+CO(g)+H2O(g) is endothermic. Would the smell of ammonia increase or decrease as the temperature is increased?
The direct reaction of iron(III) oxide. Fe2O3, to give iron and oxygen gas is a nonspontaneous reaction; normally, iron combines with oxygen to give rust (the oxide). Yet we do change iron(III) oxide, as iron ore, into iron metal. How is this possible? Explain.
Consider the reaction 2SO2(g)+O2(g)2SO3(g) (a) Calculate G at 25C. (b) If the partial pressures of SO2 and SO3 are kept at 0.400 atm, what partial pressure should O2 have so that the reaction just becomes nonspontaneous (i.e., G=+1.0 k J)?
Data in the table were collected at 540 K for the following reaction: CO(g) + NO2(g) CO2(g) + NO(g) Using the data in the table: (a) Determine the reaction order with respect to each reactant. (b) Derive the rate equation. (c) Calculate the rate constant, giving the correct units for k.

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry: An Atoms First Approach

Chemistry

ISBN:

9781305079243

Author:

Steven S. Zumdahl, Susan A. Zumdahl

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781133611097

Author:

Steven S. Zumdahl

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:

Cengage Learning

Chemistry: An Atoms First Approach

Chemistry

ISBN:

9781305079243

Author:

Steven S. Zumdahl, Susan A. Zumdahl

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781133611097

Author:

Steven S. Zumdahl

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Chemistry: Principles and Practice

Chemistry