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 1.90 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

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 1.90 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

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 data in the table, calculate the standard entropy changes for the following reactions at 25°C. S(s) + O2(g) → S02(g) Species [J/(mol K)] S(s) 167.83 J/(mol K) O2(g) 205.15 MGCO3(s) → MgO(s) + CO2(g) SO,(g) 248.22 MGCO3(s) 65.7 J/(mol K) MgO(s) 27.0 CO28) 213.78 2 C,H,(g) + 7 O2g)→ 4 CO2(g) + 6 H2O(1) C;Hg) 229.16 J/(mol K) H,0() 69.95
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)
Acetone, CH; COCH3 , boils at 56°C. The heat of vaporization of acetone at this temperature is 29.1 kJ/mol. What is the entropy change when 9 mol of liquid acetone vaporizes at 56°C?
Without doing any calculations, determine the sign of AS and ASu for each chemical reaction. In addition, predict under what temperatures (all temperatures, low temperatures, or high temperatures), if any, the reaction is spontaneous. a. 2 CO(g) + O2(g) 2 CO,(g) AHn = -566.0 kJ b. 2 NO,(g) 2 NO(g) + O,(g) AHan = +113.1 kJ c. 2 H,(g) + 0,(g) 2 H,0(g) d. CO,(g) - C(s) + O2(g) AHn = -483.6 kJ AHsn = +393.5 kJ Exn
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)…
The decomposition of nitrogen pentoxide in the reaction 2N₂O5 (s)→ 4NO2(g) + O2(g) is endothermic with AH = +110 kJ/mol. Even so, this reaction is spontaneous for temperatures above 230 K because the change of a solid into a gas is a large increase of entropy.
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
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?
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
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)