Analyze the table below. According to the table, if a process is spontaneous and has a positive AS, what must be true of its enthalpy change, AH? Enthalpy Change Entropy Change Spontaneous Reaction? Exothermic (-AH) Increase (+AS) | Yes, -AG at any temperature Exothermic (-AH) Decrease (-AS) | Only at low temps, if |T AS| < JAH| Endothermic (+AH) | Increase (+AS) Only at high temps, if |T AS| > |AH| Endothermic (+AH) | Decrease (-AS) No, +AG at any temperature AH must be positive. AH must be negative. C There is no way to know the enthalpy change. The enthalpy change depends on temperature.

Analyze the table below. According to the table, if a process is spontaneous and has a positive AS, what must be true of its enthalpy change, AH? Enthalpy Change Entropy Change Spontaneous Reaction? Exothermic (-AH) Increase (+AS) | Yes, -AG at any temperature Exothermic (-AH) Decrease (-AS) | Only at low temps, if |T AS| < JAH| Endothermic (+AH) | Increase (+AS) Only at high temps, if |T AS| > |AH| Endothermic (+AH) | Decrease (-AS) No, +AG at any temperature AH must be positive. AH must be negative. C There is no way to know the enthalpy change. The enthalpy change depends on temperature.

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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A mole of sodium met is added to water How much work is done on the atmosphere by the subsequent reaction if the temperature is 25 C°
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The following graph shows data collected for the reaction. 2 NO2 (g) = 2 NO (g) + O2 (g). y = -13704x + 75.0423 4 2 InKeq -2 -4 -6 -8 0.005 0.0052 0.0054 0.0056 0.0058 0.006 1/T (K) a) Calculate the standard changes in enthalpy, entropy, and Gibb's free energy for the reaction at 425 K. b) What effect (if any) does this reaction have on the entropy of the surroundings? Explain in one sentence.
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A chemical engineer 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 136.0 °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 = -2220, kJ J AS = -5426. K C,H, (g) + 50,(8) → 3C0,g) + 4H,0() AG = kJ Which is spontaneous? O this reaction O the reverse reaction O neither ΔΗ 50. ky AS = 6CI, (g) + 2Fe,0.(s)…
For the reaction C(s,graphite) + 02(g) CO2(g) AG° = -394.3 kJ and AS° = 2.9 J/K at 290 K and 1 atm. This reaction is (reactant, product) favored under standard conditions at 290 K. The standard enthalpy change for the reaction of 2.38 moles of C(s,graphite) at this temperature would be kJ.
Enthalpy and Gibb's Free Energy Chemical energy is released or absorbed from reactions in various forms. The most easily measurable form of energy comes in the form of heat, or enthalpy. The enthalpy of a reaction can be calculated from the heats of formation of the substances involved in the reaction: AHxn = AH₂ (products) - AH (reactants) Entropy change, AS°, is a measure of the number of energetically equivalent microstates introduced into the system during the reaction. The degree of spontaneity of a reaction is represented by the Gibbs free energy, AGO. The Gibbs free energy depends on both the enthalpy and entropy changes that take place during the reaction: AG=AH° - TAS° where T is standard temperature, 298 K. ▼ Part A Calculate the standard enthalpy change for the reaction where the heats of formation are given in the following table: ΔΗ Substance (kJ/mol) A B C D -241 -407 191 -501 Express your answer in kilojoules. ► View Available Hint(s) {—| ΑΣΦ AHixn= 2A+B=2C+2D ? kJ…