Consider the reaction 2NO(g) + 2H₂(g) N₂(g) + 2H₂O(1) 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 1.549 moles of NO(g) react under standard conditions at 298.15 K. Suniverse = (2) Is this reaction reactant or product favored under standard conditions? ✪ J/K (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'. C

Consider the reaction 2NO(g) + 2H₂(g) N₂(g) + 2H₂O(1) 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 1.549 moles of NO(g) react under standard conditions at 298.15 K. Suniverse = (2) Is this reaction reactant or product favored under standard conditions? ✪ J/K (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'. C

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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Determine the universe entropy change ΔS° (universe) in J/K (with 4 significant figures) for the reaction below at 298.15 K. Note that the temperature of surroundings is also 298.15 K. I2(s) + 3Cl2 (g) → 2 ICl3 (s) The standard entropy change and enthalpy change of the reaction (from the system) are given below: ΔS° (reaction) = -450.33 J/K and ΔH° (reaction) = -179.16 kJ
For a particular reaction, ΔH = -32 kJ and ΔS = -98 J/K.Assume that ΔH and ΔS do not vary with temperature.(a) At what temperature will the reaction have ΔG = 0?(b) If T is increased from that in part (a), will the reactionbe spontaneous or nonspontaneous?
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
For the following reaction (the detonation of nitroglycerin), is it spontaneous under standard conditions and how can you tell? 4 C4H5N3O9(l) (arrow >) 12 CO2(g) + 10 H2O(g) + 6 N2(g) + O2(g) ΔH = -5678 kJ
Consider the reaction 6CO2(g) + 6H20((1) C,H12O6 + 602(g) for which AH° = 2.801×10° kJ and AS° = -259.0 J/K at 298.15 K. (1) Calculate the entropy change of the UNIVERSE when 1.722 moles of CO2(g) 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'.
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)
Consider the following reaction: C(graphite) + 1/2 O2 (g) → CO(g) Is it spontaneous under standard conditions at 298 K? Answer this question by calculating AS" (system), AS° (surroundings), and AS (universe). (Define reactants and products as the system.) S* (J/mol · K) A¡H° (kJ/mol) at 298 K (kJ/mol) Compound at 298 K C(s, graphite) 5.6 CO(g) 197.674 -110.525 CS2 (g) 237.8 116.7 CCL (e) 214.39 -128.4 Cl2 (g) 223.08 Si(s) 18.82 SİCL, (g) 330.86 -662.75 S(s, rhombic) 32.1 Br2 (e) 152.2 HBr(g) 198.70 -36.29 H2 (g) 130.7 H2O2 (e) 109.6 -187.78 O2 (g) 205.07 O yes O no
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See image for question. Please answer with units of kJ.
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)
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