) Determine the standard enthalpy change and std. Gibbs free energy change ofreaction at 400 k for the reactionCo(g) +2H2(g) → CH;OH (g)At 298.15 K, AH?,co (»= -26.41 kcal/mol, AH9,cH,0H(0)= -48.08 kcal/mol,AG,co ()= -32.8079 kcal/mol, AG?.cH,oH()= -38.69 kcal/mol,The standard heat capacity of various components is given by,C = a + bT + cT² + dT³, where C§ is in cal/mol-K and T is in K|ComponentCH;OHCOb x10с х105-0.2910.1283ad ×10"4.556.7262.1860.04-0.0457-1.92-0.5307-0.20796.9520.09563

Answered: Image /qna-images/answer/88109b5d-94fc-4562-b3d4-afb81c5ed1ef.jpg

Determine the standard enthalpy change and std. Gibbs free energy change of reaction at 400 k for the reaction Cog) +2H:(g) → CH,OH (g) At 298.15 K, AH?.co = -26.41 kcal/mol, AH? cn,on)= -48.08 kcal/mol, AG?co m)= -32.8079 kcal/mol, AG,cn,on)= -38.69 kcal/mol, The standard heat capacity of various components is given by, C = a + bT + cT² + dT³, where Cf is in cal/mol-K and T is in K b x10 2.186 0.04 Сomponent CHOH e x10 d x10 4.55 6.726 -1.92 -0.291 0.1283 -0.5307 -0.2079 CO H2 6.952 -0.0457 0.09563

Determine the standard enthalpy change and std. Gibbs free energy change of reaction at 400 k for the reaction Cog) +2H:(g) → CH,OH (g) At 298.15 K, AH?.co = -26.41 kcal/mol, AH? cn,on)= -48.08 kcal/mol, AG?co m)= -32.8079 kcal/mol, AG,cn,on)= -38.69 kcal/mol, The standard heat capacity of various components is given by, C = a + bT + cT² + dT³, where Cf is in cal/mol-K and T is in K b x10 2.186 0.04 Сomponent CHOH e x10 d x10 4.55 6.726 -1.92 -0.291 0.1283 -0.5307 -0.2079 CO H2 6.952 -0.0457 0.09563

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter16: Thermodynamics: Directionality Of Chemical Reactions

Section: Chapter Questions

Problem 89QRT: Determine the standard Gibbs free energy change, rG, for the reactions of liquid methanol, of CO(g),...

See similar textbooks

Similar questions

Determine the standard Gibbs free energy change, rG, for the reactions of liquid methanol, of CO(g), and ofethyne, C2H2(g), with oxygen gas to form gaseous carbondioxide and (if hydrogen is present) liquid water at298 K. Use your calculations to decide which of thesesubstances are kinetically stable and which are thermodynamically stable: CH3OH(), CO(g), C2H9(g), CO2(g),H2O().
Another step in the metabolism of glucose, which occurs after the formation of glucose6-phosphate, is the conversion of fructose6-phosphate to fructose1,6-bisphosphate(bis meanstwo): Fructose6-phosphate(aq) + H2PO4(aq) fructose l,6-bisphosphate(aq) + H2O() + H+(aq) (a) This reaction has a Gibbs free energy change of +16.7 kJ/mol of fructose6-phosphate. Is it endergonic or exergonic? (b) Write the equation for the formation of 1 mol ADP fromATR for which rG = 30.5 kJ/mol. (c) Couple these two reactions to get an exergonic process;write its overall chemical equation, and calculate theGibbs free energy change.
a) Describe in your own words the relationship between standard change in Gibbs free energy associated with a chemical process (∆?o) and an equilibrium constant, Keq. A ∆?o of –3.8 kJ/mol is associated with the equilibrium 2A+B⇌C+D. If A and B are initially present in 1M concentration, find the equilibrium concentrations of all species. You know this reaction to be spontaneous at all temperatures, what can you deduce about the signs of the changes in enthalpy and entropy associated with this process? Why?
Calculate the enthalpy of solution for the dissolution of lithium iodide, LiI, molar mass = 133.85 g mol-1. When 1.49 g of LiI is dissolved in a coffee cup calorimeter containing 75.0 mL of water the temperature increased from 23.5 °C to 25.7 °C. The specific heat of water is 4.184 J g-1 °C-1, and assume the density of the solution is 1.00 g mL-1. -62 kJ mol-1 -39 kJ mol-1 30 kJ mol-1 -76 kJ mol-1 18 kJ mol-1
Given the following standard enthalpies of hydration; Mg 2 + (g) + (ag) Mg2+(aq); A110 - 1920KJ C-n (g) + (aq) CT (a q) ; All 0 - 364 KJ- and using the value of AHO for the reaction a!ready given; calculate the standard enthalpy of solution of magnesium chloride.
Certain bacteria in the soil obtain the necessary energy for growth by oxidizing nitrite to r nitrate: 2NO2- (aq) + O2(g) —> 2NO3-(aq) Given that the standard Gibbs energies of formation of NO2- and NO3- are -34.6 kJ mol-1 and -110.5 kJ mol-1, respectively, calculate the amount of Gibbs energy released when 1 mole of No2- is oxidized to 1 mole of NO3-.
A coffee-cup (constant pressure) calorimeter is used to carry out the following reaction in 63.5 mL water (where X is a hypothetical metal): X + 2 HCl → XCl2 + H2 In this process, the water temperature rose from 25.0 °C to 34.1 °C. If 0.00618 mol of "X" was consumed during the reaction, what is ΔrH of this reaction in kJ mol-1 with respect to "X"? The specific heat of water is 4.184 J g-1 °C-1 Express in 2 sig digs!
To a test tube containing 10.0 ml of 0.50 M HCl solution in a calorimeter, 0.05482 g of solid MgO (MW = 40.30 g/mol) at the same temperature was added. A change in temperature of 6.2°C was recorded. In a separate experiment, the heat capacity of the calorimeter was determined to be 0.293 kJ/°C. 1. Write the balanced equation for the reaction between HCl and MgO.2. Which is the limiting reactant? Show your solution.3. Calculate heat released by the reaction, qrxn, in the calibration step (in kJ).
Use ∆Hf0 of CO2 and H2O and combustion enthalpy of sucrose (6.155 x 103 kJmol-1 ) to calculate ∆Hf0 of sucrose
What is the entropy at SATP of a reaction where ∆Hºrxn=12.5 kJ and Keq=32.1?
The standard enthalpy of combustion of the solid glycine (the amino acid, NH2CH2COOH) is −969 kJ mol−1 at 298 K and its standard molar entropy is 103.5 J K−1 mol−1. Calculate the standard Gibbs energy of formation of glycine at 298 K. Note that the nitrogen-containing species produced on combustion is taken to be N2(g).
Suppose a certain small bird has a mass of 30 g. What is the minimum mass of glucose that it must consume to fly to a branch 10 m above the ground? The change in Gibbs energy that accompanies the oxidation of 1.0 mol C6H12O6(s) to carbon dioxide and water vapour at 25 °C is -2828 kJ.