3Fe,O3(s) + H2(g)→2Fe3O4(s) + Hz0(g) for which AH° = -6.000 kJ and AS° = 88.70 J/K at 298.15 K. (1) Calculate the entropy change of the UNIVERSE when 1.575 moles of Fe,O3(s) react under standard conditions at 298.15 K. ASuniverse |J/K (2) Is this reaction reactant or product favored under standard conditions? (3) If the reaction is product favored, is it enthalpy favored, entropy favored, or favored by both enthalpy and entropy? If the reaction is reactant favored, choose 'reactant favored'.

3Fe,O3(s) + H2(g)→2Fe3O4(s) + Hz0(g) for which AH° = -6.000 kJ and AS° = 88.70 J/K at 298.15 K. (1) Calculate the entropy change of the UNIVERSE when 1.575 moles of Fe,O3(s) react under standard conditions at 298.15 K. ASuniverse |J/K (2) Is this reaction reactant or product favored under standard conditions? (3) If the reaction is product favored, is it enthalpy favored, entropy favored, or favored by both enthalpy and entropy? If the reaction is reactant favored, choose 'reactant favored'.

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...

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Consider the reactionCa(OH)2(aq) + 2HCl(aq)CaCl2(s) + 2H2O(l)for which H° = -30.20 kJ and S° = 205.9 J/K at 298.15 K.(1) Calculate the entropy change of the UNIVERSE when 2.325 moles of Ca(OH)2(aq) react under standard conditions at 298.15 K.Suniverse = J/K(2) Is this reaction reactant or product favored under standard conditions?(3) If the reaction is product favored, is it enthalpy favored, entropy favored, or favored by both enthalpy and entropy? If the reaction is reactant favored, choose 'reactant favored'.
Do not give handwriting solution. Calculate the entropy change, ΔS, for the following processes. If needed, Cp(O2)= 29.4 J mol-1 K-1 and Cp(CO2) = 37.1 J mol-1 K-1.(a) The pressure of one mole of O2(g) is increased from P to 2P at 298 K.(b) The temperature of one mole of CO2(g) is increased from 298 K to 355 K at aconstant volume of 20.0 L.
Calculate the standard entropy of formation of liquid ethanol at 25°C. [S0(Cgraphite) = 160.70J/K•mol, S0(O2) = 205.14 J/K•mol, S0(H2) = 130.68 J/K•mol, S0(C2H5OH) = 130.68 J/K•mol]
If AS at 25°C sys =-198.3 J/K, is the reaction spontaneous N2 + 3H2 → 2NH3 • AS univ = AS sys + AS surr > ? AS surr (AHsys)/T Determine the AHrxn • AH° N2(g) = 0 kJ/mol • AH° H2(g) = 0 kJ/mol • AH°; NH3(g) = -46.19 kJ/mol
5-For the reaction, A+B C, AH-+30 kJ; AS°=+50 J/K.Therefore the reaction is: (a) spontaneous at all temperatures. (b) nonspontaneous at all temperatures. (d) irreversible at all temperatures (c) reversible at all temperatures 6- How much heat is necessary to convert 2mol of water at( 50°C) to steam at 150°C?The molar heat capacity of liquid water and steam are 75.3 J/mol. K and 36.4 J/mol. K respectively. The heat of vaporization 40.7 KJ/mol. a-81400J 7- From the reactions: b-82.337KJ c-753J d-3641 e- none of them Cgraphia +2H2(g) → CHA(R) AH = -79.9KJ C(graphia + 2Cl2(g) → CCla AH = -139KJ H 20 + Cl₂00) → HCL) AH-92.3KJ 202) calculate AH, for the reaction CH ACE +4Cl2) a- (-615.1KJ) c-(-428.3KJ) 4HCI+CCI b-(-311.2KJ) d- none of them
The energy produced by a spontaneous reaction is often used to provide the energy to drive nonspontaneous reactions. For example, the conversion of ATP to ADP in our cells acts as the energy source for the nonspontaneous reactions that combine amino acids during protein synthesis. Here is the conversion of ATP to ADP: ATP(aq) + H,O = ADP(aq) + HPO,²-(aq) AG° = -30.0 kj/mol A typical reaction combining two amino acids during protein synthesis has a AG = 15.0 kJ/mol. What is the minimum ATP concentration required to provide the energy to combine 1 mole of amino acid synthesis (total energy = 15.0 kJ)? Assume that the concentration of ADP = 9 µM (micromolar) and HPO42- = 4 mM (millimolar). %3! %3D
Consider the reaction 2NaOH(aq) + H2(g)—2Na(s) + 2H2O(l) for which AH° = 368.6 kJ and AS° = 15.30 J/K at 298.15 K. (1) Calculate the entropy change of the UNIVERSE when 1.759 moles of NaOH(aq) react under standard conditions at 298.15 K. ASuniverse= J/K (2) Is this reaction reactant or product favored under standard conditions? (3) If the reaction is product favored, is it enthalpy favored, entropy favored, or favored by both enthalpy and entropy? If the reaction is reactant favored, choose 'reactant favored'. Submit Answer
The decomposition of copper (1) oxide to its elements does not occur spontaneously at 375°C (AG = 140.0 kJ): Cu₂0 (s) 2 Cu (s) + 1/2O₂(g). It can be made to occur spontaneously by being coupled to the oxidation of solid carbon to form carbon monoxide gas at this same temperature (AG = -143.8 kJ): C(s) + 1/2O₂(g) → CO (g) What product(s) is/are produced as a result of coupling the two reactions? CO (g) 2 Cu (s) and 1/2 O₂ (g) 2 Cu (s) and CO (g) 2 Cu (s), 1/2 O2 (g), and CO (g) 1/2 0₂ (g)
What is the temperature at which the reaction below becomes spontaneous, if the standard entropies of reactants and products at 25oC are So (C(gr)) = 5.74 J/mol*K, So(H2(g)) = 130.68 J/mol*K, and So (C8H8(g)) = 345.2600J/mol*K and the heat of formation of C8H8(g)) is 147.8500 kJ/mol?C8H8(g) ↔ 8C(gr) + 4H2(g)a)661.88 Kb)707.958 Kc)the reaction is never spontaneousd)the reaction is always spontaneous
"M" represents a metallic element. "X" represents a nonmetallic element. Calculate ΔH for the process M3X4(s) ⟶ 3M(s) + 2X2(g) from the following information: M(s) + ½X2(g) ⟶ MX(s) ΔH°= -286.2 kJ 3MX(s) + ½X2(g) ⟶ M3X4(s) ΔH°= -84.3 kJ
AG (ky/mol) SUbStance / 1on so (ky/mol) -1206.9 /moi k) 92.9 • CaC03l>) -|128.8 • CaO (s) |- 635. I – 60 3.5 38.2 • CO2(9) - 393.5 - 394.4 213.7 191.5 3 H2(g) 202.7 ZNH3 ) -45.9 -16 193 • Hz (g) 202.7 223.0 -92.31 - 95. 30 186.79
In each of the following, use the tables of ΔHo and So to calculate ΔGo at 298 K for the reaction equation as given. 1. N2(g) + 3H2(g) → 2NH3(g) 2. Cu(s) + 1⁄2O2(g) → CuO(s)