9-10. At 298K and 100kPa, diamond and graphite's molar entropy and molar combustion heat are listed below. molar entropy S/ (J.K*mol) 2.45 A̟H„/(kJ · mol) molar combustion Diamond -395.40 Graphite 5.71 -393.51 m of the reaction graphite to diamond. 10) Which one is more stable, diamond or graphite? 9) Calculate the Atrs

9-10. At 298K and 100kPa, diamond and graphite's molar entropy and molar combustion heat are listed below. molar entropy S/ (J.K*mol) 2.45 A̟H„/(kJ · mol) molar combustion Diamond -395.40 Graphite 5.71 -393.51 m of the reaction graphite to diamond. 10) Which one is more stable, diamond or graphite? 9) Calculate the Atrs

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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E The Carnot cycle, which is a particular example of a thermodynamic cycle, allows determining the efficiency of a "heat-to-work" engine. Clausius used this to find the macroscopic definition of entropy as the heat change of the system at a particular temperature. Th and T are the high and low qh and q for the heats transferred at these temperatures. When plotted in a T-S temperatures and representation, entropy only changes in the processes (steps) where heat is added or removed. However, when plotting the Carnot cycle in the P-V representation it is clear that work is done (on or by) the system in each of the 4 processes of the cycle. a) Give the names of the 2 processes of the Carnot cycle (an engine) in which the surroundings do work on the system. Indicate the condition(s) of the walls for these processes. b) Consider the microscopic, i.e., Boltzmann's, definition of entropy for an ideal gas. Briefly discuss what needs to be satisfied so that there is no change of entropy during a…
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O ENTROPY AND FREE ENERGY Calculating dG from dH and dS A chemical engineer is studying the two reactions shown in the table below. In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 57.0 °C and constant total pressure. Then, she measures the reaction enthalpy H and reaction entropy As of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of her measurements are shown in the table. 2CH₂OH(g) + 30₂(g) 2CO₂(g) + 4H₂O(g) Complete the table. That is, calculate AG for the first reaction and As for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. 3CO₂(g) + 4H₂O(1)→ C₂H₂(g) + 50₂ (g) ΔΗ – -1353. kJ AS-4109. AG - KJ Which is…
From these two reactions at 298 K,
A chem.. ngineer is studying the two reactions shown in the table below. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 52.0 °C and constant total pressure. Then, he measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. AH = 181. kJ J AS = 557. K N, (g) + 0, (g) → 2NO (g) AG = N, (g) + 0,(8) kJ Which is spontaneous? this reaction the reverse reaction neither ΔΗ - - 1353. kJ J AS = K 2CH,OH (g) + 30,(g)…
6. A 10 kg copper block has an initial temperature of 800 K. It is placed in a well-insulated vessel containing 100 kg of water initially at 290 K. The process is isobaric at atmospheric pressure. Assume copper and liquid water have constant heat capacity of Cp = 4184 J/kg K for water and 398 J/kg-K for copper. What is the change in entropy of the universe resulting from the process? [CO3]
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1 3. Determine AS (in J K-¹ to the nearest whole number) for a system composed of 85.0 g of water that evaporates from a liquid to a gas at the normal boiling point of water. Additionally, what is AS if you evaporated twice this amount of water? (AHcondensation (H₂O) = −40.7 kJ mol−¹ ) A: 515; 1030 2-0 Ł p X-90.7) 5
Calculate ASor for the reaction 3H2(g) +N2(g) → 2NH3(g) at 744 K. Omit terms in the temperature-dependent heat capacities greater than T2/K2. CP,m(H2,g)=22.66+0.0438TK-1.0835x10-4T2K2J-K-1-mol-1 CP,m(N2,g)=30.81-0.01187TK+2.3968x10-5T2K2J-K-1.mol-1 CP,m(NH3,g)=29.29+0.01103TK+4.2446x10-5T2K2J-K-1.mol-1 H2(g) N2(g) NH3(g) So(J.mol-1 K-1) 130.7 191.6 192.8
M Preq 3 Consider the reaction 00 E D 4HCI(g) + O₂(g) 2H₂O(g) + 2Cl₂(8) for which AH° = -114.4 kJ and AS° = -128.9 J/K at 298.15 K. J/K (1) Calculate the entropy change of the UNIVERSE when 1.775 moles of HCI(g) react under standard conditions at 298.15 K. ASuniverse (2) Is this reaction reactant or product favored under standard conditions? Submit Answer (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'. 4 000 000 R F DO LO V % 5 [Review Topics] [References] Use the References to access important values if needed for this question. T Retry Entire Group 8 more group attempts remaining Cengage Learning Cengage Technical Support G 6 B Y H & 7 N U 1 * 8 J M 9 K बैं O < L P Previous Email Instructor Save and Exit { + 11 Next ? } ]
b) i. Define entropy. ii. 1.0 kg of water at 0 °C is mixed with an equal mass of water at 100 °C. After equilibrium is reached, the mixture has a uniform temperature of 50 °C. Calculate the change in entropy of the water. R= 8.31 kJ mol- K- and for water, Cy = 4186 J kg' K'.