Determine if the redox reaction of iron and water to form ferric chloride is spontaneous at 29°C.Chemical Equation: Fe + H20 → Fe3O4 + H21. Compute for the AG of the equation:_kJ/mol (Supply answer up to the 1st decimal point)CompoundFeH20Fe304H2AH° (kJ/mol)AS° (J/K•mol)27.2-285.869.91118.4145.2131

Answered: Image /qna-images/answer/cda6bede-6cf8-4249-a767-fed2b372c8e3.jpg

Determine if the redox reaction of iron and water to form ferric chloride is spontaneous at 29°C. Chemical Equation: Fe + H20 FezO4 + H2 1. Compute for the AG of the equation: _kJ/mol (Supply answer up to the 1st decimal point) Compound Fe AH° (kJ/mol) AS° (J/K•mol) 27.2 H20 Fe304 H2 -285.8 69.9 1118.4 145.2 131

Determine if the redox reaction of iron and water to form ferric chloride is spontaneous at 29°C. Chemical Equation: Fe + H20 FezO4 + H2 1. Compute for the AG of the equation: _kJ/mol (Supply answer up to the 1st decimal point) Compound Fe AH° (kJ/mol) AS° (J/K•mol) 27.2 H20 Fe304 H2 -285.8 69.9 1118.4 145.2 131

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter16: Spontaneity Of Reaction

Section: Chapter Questions

Problem 84QAP: Determine whether each of the following statements is true or false. (a) An exothermic reaction is...

See similar textbooks

Similar questions

Many biochemical reactions that occur in cells require relatively high concentrations of potassium ion (K+). The concentration of K + in muscle cells is about 0.l5 M. The concentration of K+ in blood plasma is about 0.0050 M. The high internal concentration in cells is maintained by pumping K+ from the plasma. How much work must be done to transport 1.0 mole of K+ from the blood to the inside of a muscle cell at 37C, normal body temperature? When 1.0 mole of K+ is transferred from blood to the cells, do any other ions have to be transported? Why or why not?
For the reaction NO(g)+NO2(g)N2O3(g) , use tabulated thermodynamic data to calculate H and S. Then use those values to answer the following questions. (a) Is this reaction spontaneous at 25°C? Explain your answer. (b) If the reaction is not spontaneous at 25°C, will it become spontaneous at higher temperatures or lower temperatures? (c) To show that your prediction is accurate, choose a temperature that corresponds to your prediction in part (b) and calculate G . (Assume that both enthalpy and entropy are independent of temperature.)
Nickel metal reacts with carbon monoxide to form tetra-carbonyl nickel, Ni(CO)4: Ni(s)+4CO(g)Ni(CO)4(g) This reaction is exploited in the Mond process in order to separate pure nickel from other metals. The reaction above separates nickel from impurities by dissolving it into the gas phase. Conditions are then changed so that the reaction runs in the opposite direction to recover the purified metal. (a) Predict the sign of S for the reaction as written above. (b) Use tabulated thermodynamic data to calculate H, S , and G for the reaction. (c) Find the range of temperatures at which this reaction is spontaneous in the forward direction.
The reaction shown below is involved in the refining of iron. (The table that follows provides all of the thermodynamic data you should need for this problem.) 2Fe2O3(s)+3C(s,graphite)4Fe(s)+3CO2(g) (a) Find H for the reaction. (b) S for the reaction above is 557.98 J/K. Find S° for Fe2O3(s). (c) Calculate G for the reaction at the standard temperature of 298 K. (There are two ways that you could do this.) (d) At what temperatures would this reaction be spontaneous? Compound Hf (kJ mol-1) S° (kJ mol-1) Gf (J mol-1 K-1) Fe2O3(s) -824.2 ? -742.2 C(s, graphite) 0 5.740 0 Fe(s) 0 27.3 0 CO2(g) -393.5 213.6 -394.4.83
For the reaction C2H2(g)+4F2(g)2CF4(g)+H2(g) S is equal to 358 J/K. Use this value and data from Appendix 4 to calculate the value of S for CF4(g).
Use the data in Appendix G to calculate the standard entropy change for H2(g) + CuO(s) H2O() + Cu(s)
For the reaction TiCl2(s) + Cl2(g) TiCl4(), rG = 272.8 kj/mol-txn. Using this value and other data available in Appendix L, calculate the value of fG for TiCl2(s).
Given the following data 2O3(g) 3O2(g)H = 427 kJ O2(g) 2O(g)H = 495 kJ NO(g) + O3(g) NO2(g) + O2(g)H = 199 kJ Calculate H for the reaction NO(g) + O(g) NO2(g)
Methane can be produced from CO and H2.The process might be done in two steps, as shown below, with each step carried out in a separate reaction vessel within the production plant. Reaction 1 CO(g)+2H2(g)CH3OH(l) S = -532 J/K Reaction 2 CH3OH(l)CH4(g)+12O2(g) S= +162 J/K NOTE: You should be able to work this problem without using any additional tabulated data. (a) Calculate H for reaction 1. (b) Calculate Gf for CO(g). (c) Calculate S° for O2(g). (d) At what temperatures is reaction 1 spontaneous? (e) Suggest a reason why these two steps would need to be carried out separately. Substance Hf (kJ mol-1) Gf (kJ mol-1) S (J mol-1 K-1) CO(s) -110.5 197.674 CH3OH( l ) -238.7 -166.4 126.8 CH4(g) -74.8 186.2
A bottle of soda has a head space containing 25.0 mL of CO2 gas at 4.2 atm pressure when the soda is at 4.4C. The bottle is opened slowly, letting the excess pressure escape. Howmuch work does the escaping CO2 do if the ambient pressure is 1.0 atm? Assume that the temperature remains constant.
Define the standard enthalpy of formation. What are standard states for elements and for compounds? Using Hess's law, illustrate why the formula Hreaction=npHf(products)nfHf(reactants) works to calculate H for a reaction.
For a process, w = 34 J and q = 109 J. What is E for this process?