The standard-state Gibbs free energy change (AGO) for a process can be defined as: AG=AHⓇ - TAS°, where AH° is the standard-state enthalpy change, T is the absolute temperature in units of Kelvin, and AS is the standard-state entropy change. A plot of AG° (y-axis) versus T (x axis) for a hypothetical process is shown below. The line of best fit for the data is y = -0.5x + 100. AG (kJ/mol) 100 50 AH° = 0 -100 AS° = -50 -150 0 100 200 300 400 500 What are the values (including the correct signs) of AH and AS for this process? y=-0.5x+100 T(K) choose your answer... choose your answer...

The standard-state Gibbs free energy change (AGO) for a process can be defined as: AG=AHⓇ - TAS°, where AH° is the standard-state enthalpy change, T is the absolute temperature in units of Kelvin, and AS is the standard-state entropy change. A plot of AG° (y-axis) versus T (x axis) for a hypothetical process is shown below. The line of best fit for the data is y = -0.5x + 100. AG (kJ/mol) 100 50 AH° = 0 -100 AS° = -50 -150 0 100 200 300 400 500 What are the values (including the correct signs) of AH and AS for this process? y=-0.5x+100 T(K) choose your answer... choose your answer...

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 chemicai 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 42.0 °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. ΔΗ Ξ - 70. kJ J AS = -151. K TiCl, (g) + 2H,0(g) → Tio, (s) + 4H Cl (g) AG = || kJ Which is spontaneous? this reaction the reverse reaction neither AH = 439. kJ AS = K 4H,PO, (s) →…
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A system consists of 50.0 g of liquid water. The water is vaporized to form steam at 1.00 bar and 100.°C. How much work (in kJ) is done by the system during this process? The density of liquid water is 0.959 g mL−1 at 100.°C.
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…
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