[References] Calculate AS for the following reactions, using standard entropy values from the table below. a. For the reaction 4Al(s) + 302(9) → 2Al,O3(s) Species S° J/(mol-K) Al(s) 28.28 O2 (9) 205.0 Al, O3 (s) 50.95 AS = J/K

[References] Calculate AS for the following reactions, using standard entropy values from the table below. a. For the reaction 4Al(s) + 302(9) → 2Al,O3(s) Species S° J/(mol-K) Al(s) 28.28 O2 (9) 205.0 Al, O3 (s) 50.95 AS = 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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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)…
Using enthalpies of formation, calculate ΔΗ° for the following reaction at 25°C. Also calculate AS for this reaction from standard entropies at 25°C. Use these values to calculate AGO for the reaction at this temperature. Species AH (kJ/mol) S (J/mol.K) COC12 (9) H₂O(1) CO₂(g) HCl(g) ΔΗ° = AS° AGⓇ -220.1 -285.8 -393.5 -92.31 KJ J/K 283.9 kJ 69.95 COC12(g) + H₂O(1) → CO₂ (g) + 2HCl(g) 213.7 186.8
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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
Consider the following reaction: 2 H2(g) + 2 NO(g) N2(g) + 2 H20(g) and the following table of standard enthalpies of formation and standard absolute entropies: compound AH (kJ mol-1) s° (J K-1 mol-1) H2(g) 130.8 NO(g) 91.3 210.8 N2(g) 191.6 H20(g) -241.8 188.8
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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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