Consider the reaction:2NH3(g) + 3N₂O(g) → 4N₂ (g) + 3H₂O(g)Using standard absolute entropies at 298 K, calculate the entropy change for the system when 1.54 moles of NH3(g) react at standardconditions.AS⁰⁰systemSubstance So (J/K mol)NH3 (9)192.5219.9191.6188.8N₂O(g)N₂ (9)H₂O(g)J/K Consider the reaction:2BrF3 (9) → Br₂(g) + 3F2 (g)Using standard absolute entropies at 298 K, calculate the entropy change for the system when 2.27 moles of BrF3 (g) react at standardconditions.AsosystemSubstance SoBr₂(g)F₂(g)BrF3 (9)J/KJK. mol245.5202.8292.5

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Consider the reaction: 2NH3(g) + 3N₂O(g) → 4N2₂ (g) + 3H₂O(g) Using standard absolute entropies at 298 K, calculate the entropy change for the system when 1.54 moles of NH3(g) react at standard conditions. AS⁰ system Substance So (J/K mol) NH3 (9) 192.5 N₂O(g) 219.9 N₂ (9) 191.6 H₂O(g) 188.8 J/K

Consider the reaction: 2NH3(g) + 3N₂O(g) → 4N2₂ (g) + 3H₂O(g) Using standard absolute entropies at 298 K, calculate the entropy change for the system when 1.54 moles of NH3(g) react at standard conditions. AS⁰ system Substance So (J/K mol) NH3 (9) 192.5 N₂O(g) 219.9 N₂ (9) 191.6 H₂O(g) 188.8 J/K

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 given reactions and the given molar entropy of compounds, determine whether the reaction (1) is spontaneous at normal conditions. X (1) Fe2O3(s) + 3C(graphite) 2Fe(s) + 3CO(g) (2) C(graphite) + O2(g) AHOrxn=-393.51 kJ/mol CO2(g) CO2(g) (3) CO(g) +1/2 O2(g) ΔΗ, rxn 282.98 kJ/mol. AHºf (Fe2O3(s)) = -824 kJ/(mol K) sᵒ(CO(g)) =197.7 J/(mol K) sᵒ(C(graphite)) = 5.74 J/(mol K) S°(Fe(s)) =27.3 J/(mol K) sº(Fe2O3(s)) =87.4 J/(mol K)
Consider the reaction: H₂CO(g) + O₂(g) → CO₂(g) + H₂O(1) Using standard absolute entropies at 298 K, calculate the entropy change for the system when 2.42 moles of H₂CO(g) react at standard conditions. 20 AS Substance Sº (J/K mol) H₂ CO(g) 219.0 0₂ (9) 205.1 CO₂(g) H₂O (1) 213.7 69.9 system Submit Answer 888 R V % J/K Show Hint 5 Retry Entire Group [Review Topics] [References] Use the References to access important values if needed for this question. T G B Cengage Learning | Cengage Technical Support 6 Y 9 more group attempts remaining H & 7 N U J 00 * 8 M ( 9 K 其 L E P Previous T Email Instructor Save and Exit { [ Next ? delete
11. Consider the combustion reaction of methane as shown in the following 1 point equation: * CH4 (g) + 202 (g) = CO2 (g) + 2H2O (1) By referring to the data below, compute the standard entropy changes of the reaction. Compound S (J/mol. K) CHa(g) 186.3 J/K.mol O2(g) 205 J/K.mol CO2(g) 213.6 J/K.mol H2O (1) 69.9 J/K.mol A. 37.9 J/K.mol B. -37.9 J/K.mol O C. -242.9 J/K.mol D. -107.8 J/K.mol
Standard Entropy of Reaction Molecular systems tend to move spontaneously to a state of maximum randomness or disorder. Molecular randomness, or disorder, is called entropy and is denoted by the symbol S. As a state function, entropy change, A.S. depends only on initial and final states. AS has a positive value when disorder increases and a negative value when disorder decreases. The following conditions usually result in an increase in entropy: • a change of phase: solid-liquid-gas, an increase in the number of gas molecules, or • a solid dissolving to form a solution. Although the sign of the entropy change can be predicted as described above, the actual value of AS° must be calculated from the absolute entropy values. Sº, of the reactants and products: ASS° (products) - S° (reactants) ▼ Part A Predict the sign of the entropy change. AS°, for each of the reaction displayed. Drag the appropriate items to their respective bins. ▸ View Available Hint(s) Positive Submit H₂O(1) H₂O(g)…
Calculate ASsurr and ASuniverse for a reaction. Consider the reaction H₂S(g) + 2H₂O(1)→→3H₂(g) + SO₂(g) Using standard thermodynamic data (in the Chemistry References), calculate the entropy change of the surroundings and the universe at 25°C. AS surroundings = ASuniverse J/K J/K where ASO = 294.7 J/K rxn
Consider the reaction: 4HCl(g) + O₂(g) → 2H₂O(g) + 2Cl₂ (g) Using standard absolute entropies at 298 K, calculate the entropy change for the system when 1.69 moles of HCl(g) react at standard conditions. AS⁰ Substance So (J/K mol) HCl(g) 186.9 O2(g) 205.1 H₂O(g) 188.8 Cl₂ (g) 223.1 system = J/K
Chemistry
Discuss the spontaneity of each process in the following scenarios, based on the use of the Gibbs free energy equation: 1. N₂(g) + 3H₂(g) + 2NH3(g), AH = -46.11 kJ/mol 2. An exothermic reaction with an increase in entropy 3. A block of solid carbon dioxide subliming to gaseous carbon dioxide
Methanol is burned as fuel in some race cars. This makes it clear that the reaction is spontaneous once methanol is ignited. Yet the entropy change for the reaction 2 CH3 OH (l) + 3 O2 (g) to 2 CO2 (g) + 4 H2 O(l) is negative. Why doesn't this violate the second law of thermodynamics?
5. Note: Please don't write on a paper. I can't understand handwrittens.
2 NH3 (g) + 2 O2 (g) → N20 (g) + 3 H2O (g) Is this reaction spontaneous only at low temperatures, only at high temperatures, at all temperatures? AH°r, kJ/mol s°, J/mol·K NH3(g) -46.1 192.5 0:(g) 205.0 N 20 (g) 82.1 219.9 H2O(g) |-241.8 188.7 AH°i, kJ/mol s°, J/mol·K What is the lowest temperature at which the following reaction is spontaneous? H2O (g) + C (s) → H2 (g) + CO (g) Co(g) H2(g) C (s) -110.5 | 197.7 130.6 5.7 H2O(g) |-241.8 188.7
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