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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Consider the reactionCa(OH)2(aq) + 2HCl(aq)CaCl2(s) + 2H2O(l)for which H° = -30.20 kJ and S° = 205.9 J/K at 298.15 K.(1) Calculate the entropy change of the UNIVERSE when 2.325 moles of Ca(OH)2(aq) react under standard conditions at 298.15 K.Suniverse = J/K(2) Is this reaction reactant or product favored under standard conditions?(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'.
Do not give handwriting solution. Calculate the entropy change, ΔS, for the following processes. If needed, Cp(O2)= 29.4 J mol-1 K-1 and Cp(CO2) = 37.1 J mol-1 K-1.(a) The pressure of one mole of O2(g) is increased from P to 2P at 298 K.(b) The temperature of one mole of CO2(g) is increased from 298 K to 355 K at aconstant volume of 20.0 L.
Consider each of the following reactions and decide whether the standard entropy change for the reaction will be, (a) Positive; or (b) Very close to Zero; or (c) Negative. N2 (g) + 3 H2 (g) = 2 NH3 (g) 2 Na (1) + H2 (g) = 2 NaH (s) %3D Cu (s) + 2 H2SO4 (aq) = 1. negative CusO4 (aq) + 2 H20 (1) + SO2 (g) 2. positive PCI5 (s) = PC|3 (s) + Cl2 (g) 2 v 3. very close to zero H2 (g) + Cl2 (g) = 2 HCI (g) 3. %3D BaSO4 (s) + 2 H20 (g) = %3D 1 BasO4.2H20 (s)
The energy produced by a spontaneous reaction is often used to provide the energy to drive nonspontaneous reactions. For example, the conversion of ATP to ADP in our cells acts as the energy source for the nonspontaneous reactions that combine amino acids during protein synthesis. Here is the conversion of ATP to ADP: ATP(aq) + H,O = ADP(aq) + HPO,²-(aq) AG° = -30.0 kj/mol A typical reaction combining two amino acids during protein synthesis has a AG = 15.0 kJ/mol. What is the minimum ATP concentration required to provide the energy to combine 1 mole of amino acid synthesis (total energy = 15.0 kJ)? Assume that the concentration of ADP = 9 µM (micromolar) and HPO42- = 4 mM (millimolar). %3! %3D
Consider the reaction 2NaOH(aq) + H2(g)—2Na(s) + 2H2O(l) for which AH° = 368.6 kJ and AS° = 15.30 J/K at 298.15 K. (1) Calculate the entropy change of the UNIVERSE when 1.759 moles of NaOH(aq) react under standard conditions at 298.15 K. ASuniverse= J/K (2) Is this reaction reactant or product favored under standard conditions? (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'. Submit Answer
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Consider the reaction 6CO2(g) + 6H20((1) C,H12O6 + 602(g) for which AH° = 2.801×10° kJ and AS° = -259.0 J/K at 298.15 K. (1) Calculate the entropy change of the UNIVERSE when 1.722 moles of CO2(g) react under standard conditions at 298.15 K. ASuniverse J/K (2) Is this reaction reactant or product favored under standard conditions? (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'.
For the reaction NH,NO3(aq) –→N½0(g) + 2 H2O(1) AG° = -181.7 kJ and AH° = -149.6 kJ at 321 K and 1 atm. This reaction is (reactant, product) favored under standard conditions at 321 K. The entropy change for the reaction of 2.38 moles of NH,NO3(aq) at this temperature would be J/K.
0/5 Nerbs 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 85.0 °C and constant total pressure. Then, she 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 her 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. do AH = -2220. kJ J AS = -6189 K C,H, (g) + 50, (g) 3Co, (g) + 4H,0(1) AG = KJ Which is spontaneous? O this reaction O the reverse reaction O neither AH = -50. kJ 0- AS =…
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 60.0 °C and constant total pressure. Then, she measures the reaction enthalpy ΔH and reaction entropy ΔS of the first reaction, and the reaction enthalpy ΔH and reaction free energy ΔG of the second reaction. The results of her measurements are shown in the table. Complete the table. That is, calculate ΔG for the first reaction and ΔS 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.
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