Consider the reaction 2NH3(g) + 3N₂O(g) → 4N2(g) + 3H₂O(g) for which AH-879.5 kJ and AS = 288.1 J/K at 298.15 K. 1. Calculate the entropy change of the UNIVERSE when 1.642 moles of NH3(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'.

Consider the reaction 2NH3(g) + 3N₂O(g) → 4N2(g) + 3H₂O(g) for which AH-879.5 kJ and AS = 288.1 J/K at 298.15 K. 1. Calculate the entropy change of the UNIVERSE when 1.642 moles of NH3(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'.

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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Using the provided data, determine the temperatures at which the following hypothetical reaction will be spontaneous under standard conditionsA + B → 2C + D△S°rxn = 249.1 J/K△H°rxn = 104.6 kJ * at no temperatures * at all temperatures below 146.9 °C * at all temperatures above 146.9 °C * at all temperatures above 238.1 °C * at all temperatures below 238.1 °C * at all temperatures
Consider the reaction 2NH3(g) + 3N₂O(g) → 4N₂ (9) + 3H₂O(g) for which AH° = − 879.5 kJ and AS° = 288.1 J/K at 298.15 K. 1. Calculate the entropy change of the UNIVERSE when 2.344 moles of NH3(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 element oxygen was prepared by Joseph Priestley in 1774 by heating mercury(II) oxide: HgO(s) → Hg() + 1/2O2(g), AH = 90.84 kJ/mol. Estimate the temperature at which this reaction will become spontaneous under standard state conditions. S'(Hg) = 76.02 J/K mol S(O2) = 205.0 J/K mol C S(HgO) = 70.29 J/K mol 11
A 0.576 g sample of liquid C5H12 was combusted using excess oxygen gas inside a bomb calorimeter, with the products being carbon dioxide gas and liquid water. The calorimeter's heat capacity is 4.957 kJ °C^-1. If the temperature inside the calorimeter increased from 25.0 °C to 35.1 °C, determine A,U for this reaction in kl mol (with respect to C3H12). Do not worry about how realistic the final answer is.
A sample consisting of 1.00 mol of a monatomic ideal gas at 30 ℃ is compressed reversibly and isothermally from 50.00 L to 20.00 L. Calculate the change in Helmholtz energy, ΔG (in kJ).
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Combustion of C12H22O11(s) (sucrose or "table sugar") produces CO2(g) and H2O(l). When 3.96 g of sucrose is combusted in a constant volume (bomb) calorimeter, 65.3 kJ of heat is liberated. Calculate ΔE for the combustion of 2.75g of sucrose. Calculate ΔH for the combustion of 2.75 g of sucrose.
Consider the reaction Fe(s) + 2HCl(aq) → FeCl₂ (s) + H₂(g) for which AH = -7.400 kJ and AS = 107.9 J/K at 298.15 K. 1. Calculate the entropy change of the UNIVERSE when 2.385 moles of Fe(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'. Submit Answer Retry Entire Group 5 more group attempts remaining
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A mixture of CO(g) and H2(g) is produced by passing steam over hot charcoal: H2O(g)+ C(s)->H2(g)+CO(g) Using the appropriate thermodynamic values in the table below, calculate the lowest temperature at which the reaction is spontaneous under standard conditions. Compound ΔGf (kJ/mol) ΔHf (kJ/mol) ΔHf (kJ/mol) H2O(g) –228.6 –241.8 188.8 H2O(ℓ) –237.2 –285.8 69.9 C(s) 0.0 0.0 5.7 H2(g) 0.0 0.0 130.6 CO(g) –137.2 –110.5 197.7 O2(g) 0.0 0.0 205.0 _____K
Calculate the change in entropy that occurs in the system when 1.10 mol of isopropyl alcohol (C3H§O) melts at its melting point (– 89.5 °C). AH = 5.37 kJ/mol. fus Express your answer in joules per kelvin to three significant figures.