1. Construct a pe-pH for the system Mn-02-H2O. Include the following species in the diagram: Mn2+, MnO2, Mn2O3, Mn304, and Mn(OH)2. Below is the required thermodynamic data. Species AG° (kJ/mol) Species AGr° (kJ/mol) Mn2+ -228.1 Mn3O4(s) -1282.5 MnO2(s) -453.1 Mn(OH)2(s) -616.5 Mn2O3(s) -882.1 H₂O -237.1

1. Construct a pe-pH for the system Mn-02-H2O. Include the following species in the diagram: Mn2+, MnO2, Mn2O3, Mn304, and Mn(OH)2. Below is the required thermodynamic data. Species AG° (kJ/mol) Species AGr° (kJ/mol) Mn2+ -228.1 Mn3O4(s) -1282.5 MnO2(s) -453.1 Mn(OH)2(s) -616.5 Mn2O3(s) -882.1 H₂O -237.1

Chemistry

10th Edition

ISBN:9781305957404

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

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Species AfH (kJ/mol) S (J/mol K) Mg(s) H₂O(l) Mg(OH)2 (s) H₂(g) Charles D. Winters 0 -285.83 -924.54 INCLUDES 34 Pusa S 0 32.67 Solvan Cars Mashed Porn & HEATER MEALS 69.95 63.18 130.7 HEATER MEALS . AfG (kJ/mol) 0 -237.15 -833.51 0 The heat for the heater unit is produced by the reaction of magne- sium with water. Confirm that this is a spontaneous reaction under standard conditions. Do this by calculating the value of A,Gº. What sign is expected for ArGº for a spontaneous reaction under standard conditions? A, G = kJ/mol For a spontaneous reaction under standard conditions, A, G 0.
7- Given the following data: AG --51 kJ 2H: (g) + C (s) → CHa (g) 2H2 (g) + O: (g) - 2H:0 (1) C (s) + 02 (g) → CO: (g) Calculate AG° for CH4 (g) + 202 (g)CO2 (g) + 2H;0 (). AG-474 kJ AG°--394 kJ
Calculate deltaG for the reaction /, (02) = [O]Fewto at 1650 degrees Celsius. Given: (H2) + / (02) = (H120) AG = = 251790 + 55.5T Joules (H2) + [0] Fe wt% = (H12) logk = 7040/T - 3.5 Hand written explanation
For questions 6-8 calculate the ?Hrxn based off of the given data. 6. Find ?Hrxn for S8(s) + 12O2(g) →8SO3(g)Using the thermodynamic below.S8(g) + 8O2(g) →8SO2(g) ?Hrxn= -2374 KJ2SO2(g) + O2(g)→ 2SO3(g) ?Hrxn= -792 KJ
Use the values of AH₂ Substance and State Cas (PO4)2 (8) CaSO4(s) CH₁ (9) HCN(g) HCl(g) H₂O(g) NH3 (9) NH4Cl(s) 0₂ (9) H3PO4 (1) H₂SO4 (1) a. to calculate AH for the following reactions. AH₁ (kJ/mol) -4126 -1433 -75 135.1 -92 -242 -46 -314 0 -1267 -814 N OH ΔΗ kJ b. Cas (PO4)2 (s) + 3H₂SO4 (1)→ 3CaSO4(s) + 2H3PO4 (1) AHⓇ = kJ c. NH3(g) + HCl(g) → NH4 Cl(s) AH = kJ
Calculate delta H for the following rection, FeO + CO = Fe + CO2 from the following data: Fe2O3 + 3CO --> 2Fe +3CO2 Delta H= -23 kJ 3Fe2O3 + CO --> 2Fe3O4 +CO2 Delta H= -39 kJ Fe3O4 +CO --> 3FeO +CO2 Delta H= +18 kJ
Combustion of glucose (C6H12O6) is the main source of energy for animal cells: CHO) +60, (e) 600, (e) 6H,O) + (1) rxn AG (37 °C)=-2872. kJ One of the most important uses to which this energy is put is the assembly of proteins out of amino acid building blocks. The Gibbs free energy of formation of one peptide bond, joining one amino acid to another, is 21 kJ/mol. Suppose some cells are assembling a certain protein made of 27 amino acids. (Note that the number of peptide bonds in the protein will be one less than the number of amino acids.) Calculate the minimum mass of glucose that must be burned to assemble 250. umol of this protein. Round your answer to 2 significant digits. g 0 E
c. For the reaction 2. CACO,(s) + 2H+ (aq)→ Ca (ag) + H,0(1) + CO, Species S J(mol K) CACO3 (s) 92.9 H* (ag) 0. Ca (aq) -53.1 H20(1) 69.95 CO, (9) 213.7 AS = JK
com/iln/takeAssignment/takeCovalentActivity.do?locator=assignment-take OWIV2 | Assignments | C x Use the References to access important values if needed for this question. Consider the reaction H2(g) + Ch(g)-2HCI(g) Using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15K. ANSWER: Submit Answer Retry Entire Group 9 more group attempts remaining (Previous Next Save and Exit 11:47 AM 11/9/2020 AAA prt sc delete hom backspace
This question has multiple parts. Work all the parts to get the most points. Calculate AH for the reaction 2K() + 2H,О(1)- 2КОН(ад) + На (9) Substance and State AH (kJ/mol) K(s) KOH(aq) H2(g) H20(1) -481 -286 ΔΗ -390 kJ %3D bA 5.50-g chunk of potassium is dropped into 1.00 kg water at 24.6°C. What is the final temperature of the water after the preceding reaction occurs? Assume that all the heat is used to raise the temperature of the water. (Never run this reaction. It is very dangerous; it bursts into flame!) Temperature = Submit
a Calculate AH° for the reaction 2K(s) + 2H,O(1) - - 2KOH(aq) + Hz2 (9) Substance and State AH° (kJ/mol) K(s) KOH(aq) H2 (9) H2O(1) -481 -286 AH° = -390 kJ bA 5.20-g chunk of potassium is dropped into 1.00 kg water at 24.2°C. What is the final temperature of the water after the preceding reaction occurs? Assume that all the heat is used to raise the temperature of the water. (Never run this reaction. It is very dangerous; it bursts into flame!) Temperature = °C Submit
[References] |Substance and State AH£° (kJ/mol) | Саз (РОд)2(8) CaSO4 (s) CH4 (9) HCN(g) HCI(g) H2O(g) NH3 (g) NHẠ CI(s) O2 (9) H3PO4 (1) H2SO4 (1) -4126 -1433 -75 135.1 -92 -242 -46 -314 -1267 -814 а. (g) + (g) + (g) + (g) N ΔΗ'- kJ b. Сaз (РО,), (8) + зн;SO4(1) —— зСaSO, (s) + 2H3PОД (1) ΔΗ' kJ с. NH3 (9) + HCI(9) — NH4 CI(s) ΔΗ' kJ Previous