Consider the reaction2NO(g) + 2H2(g)-→N2(g) + 2H2O(I)for which AH° = -752.2 kJ and AS° = -351.6 J/K at 298.15 K.(1) Calculate the entropy change of the UNIVERSE when 2.388 moles of NO(g) react under standard conditions at 298.15 K.ASuniverseJ/K%3D(2) Is this reaction reactant or product favored under standard conditions?reactant(3) If the reaction is product favored, is it enthalpy favored, entropy favored, or favored bnalpy and entropy? If the reaction is reactant favored choose 'reactant favored'.product

Given information, ∆H° = -752.2 kJ ∆S° = -351.6 J/K (at 298.15 K)

Consider the reaction 2NO(g) + 2H2(g) N2(g) + 2H2O() for which AH° = -752.2 kJ and AS° = -351.6 J/K at 298.15 K. (1) Calculate the entropy change of the UNIVERSE when 2.388 moles of NO(g) react under standard conditions at 298.15 K. ASuniverse = J/K (2) Is this reaction reactant or product favored under standard conditions? reactant (3) If the reaction is product favored, is it enthalpy favored, entropy favored, or favored b halpy and entropy? If the reaction is reactant favored choose 'reactant favored'. product

Consider the reaction 2NO(g) + 2H2(g) N2(g) + 2H2O() for which AH° = -752.2 kJ and AS° = -351.6 J/K at 298.15 K. (1) Calculate the entropy change of the UNIVERSE when 2.388 moles of NO(g) react under standard conditions at 298.15 K. ASuniverse = J/K (2) Is this reaction reactant or product favored under standard conditions? reactant (3) If the reaction is product favored, is it enthalpy favored, entropy favored, or favored b halpy and entropy? If the reaction is reactant favored choose 'reactant favored'. product

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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calculate ΔS rxn (standrad entropy) and Δ Ssurr for the reactions and determine if each is spontaneous at 25 degrees celsius.
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Consider the reaction2H2S(g) + 3O2(g)2H2O(l) + 2SO2(g)for which H° = -1.124×103 kJ and S° = -390.7 J/K at 298.15 K.(1) Calculate the entropy change of the UNIVERSE when 2.296 moles of H2S(g) 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'.
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'.
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
Calculate the change of the entropy of the system in J/K for the following phase transition: vaporization of 159.2 g propanol The molar mass of n-propanol (C3H7OH) is 60.095 g/mol; the enthalpy of vaporization of n-propanol is 47.5 kJ/mol; the boiling point of n-propanol is 97.7°C Group of answer choices 128 -486 -339 1280 0.3393
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)
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For a particular chemical reaction H = 6.8 kJ and S = –29 J/K. Under what temperature condition is the reaction 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