Gibbs free energy (G) is a measure of the spontaneity of a chemical reaction. It is the chemical potential for a reaction, and is minimized at equilibrium. It is defined as G=H-TS where H is enthalpy, T is temperature, and Sis entropy. The chemical reaction that causes iron to corrode in air is given by 4Fe+302-2Fe2O3 in which at 298 K, AH = ASixn= -543.7 J/K. 1684 kJ and Part A What is the standard Gibbs free energy for this reaction? Assume the commonly used standard reference temperature of 298 K. Express your answer as an integer and include the appropriate units. ▸ View Available Hint(s) μÅ AGxn= Value Submit n C Units ?

Gibbs free energy (G) is a measure of the spontaneity of a chemical reaction. It is the chemical potential for a reaction, and is minimized at equilibrium. It is defined as G=H-TS where H is enthalpy, T is temperature, and Sis entropy. The chemical reaction that causes iron to corrode in air is given by 4Fe+302-2Fe2O3 in which at 298 K, AH = ASixn= -543.7 J/K. 1684 kJ and Part A What is the standard Gibbs free energy for this reaction? Assume the commonly used standard reference temperature of 298 K. Express your answer as an integer and include the appropriate units. ▸ View Available Hint(s) μÅ AGxn= Value Submit n C Units ?

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 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 37.0 °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. 6C(s) + 6H₂(g) + 30₂(g) → CH₁₂O6 (s) CH₂OH(g) + CO(g) → HCH₂CO₂ (1) ΔΗ = -1237. kJ J K AS-3953. AG = KJ Which is spontaneous? O this reaction. O the reverse reaction O neither ΔΗ = −…
Calculate the entropy change in surroundings when 1.00 mol of H:0 (1) is formed under standard conditions, A:H = -286 kJmol1. Industrially, methanol is synthesized using the reaction Co(e) + 2 H2(g) =CH:OH(g) Calculate the equilibrium constant at 298 K. AGP CO(g) = -137.2 kJ/mol; AGP H: (g)= 0; AGP CH:OH(g) = -162 kJ/mol
Calculate AHxn for the reaction 2Ni(s) + 25(s) + 30,(g) – → 2NISO, (s) from the following information: 1. Niso,(s) - Nio(s) + So,(g) = 156 kJ rxn 2. s(s) + 0,(3) so, (g) AH° =-297 kJ fxn 3. Ni(s) + 0,(g) → Nio(s) AH° =-241 kJ rxn AH pn= kJ
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 72.0 °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. C₂H₂(g) + 50₂(g) → 3CO₂(g) + 4H₂O(1) 2CO₂ (g) + 4H₂O(g) → 2CH, OH (g) + 30₂ (g) ΔΗ = -1220. ΚΙ J K AS-6432. AG - KJ Which is spontaneous? O this reaction O the reverse reaction…
Predict if the reaction happens spontaneously by calculating the standard entropy (ASrxn), entropy of the surroundings (ASsurr), and entropy of the universe (ASuniv) of the reaction at 250C: Hz(g) + CuO(s)_ + Cu(s) + H20(g) AHre= -86.6 kJ
Using enthalpies of formation, calculate AH° for the following reaction at 25°C. Also calculate AS" for this reaction from standard entropies at 25°C. Use these values to calculate AG for the reaction at this temperature. Species AH; (kJ/mol) S" (J/mol·K) COCL, (9) -220.1 283.9 H20(1) -285.8 69.95 CO2 (9) -393.5 213.7 HCI(9) -92.31 186.8 COCI, (9) + H20(1) + CO, (9) + 2HCI(9) ΔΗ' kJ AS J/K AG° = kJ
In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 72.0 °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. P₂010 (s) + 6H₂0 (1) 4H₂ PO(s) 4 2NH₂ (g) → N₂H₂(g) + H₂ (g) 2 4 2 ΔΗ = -439. kJ AS-1179. AG = AH = k AS = kJ Which is spontaneous? this reaction the reverse reaction neither 188. kJ OK- K J K AG 16. kJ Which is spontaneous? this reaction the reverse…
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 114.0 °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. ol. Ar AH = 852. kJ J AS = 2176. Al, 0, (s) + 2Fe(s) → 2 A1(s) + Fe,0, (s) AG = | kJ Which is spontaneous? this reaction the reverse reaction neither
Given the reactions, ΔΗ 891.5 kJ X(s) +0,(g) - XO(s) X0(s) + CO,(g) XCO,(s) +494.5 kJ ΔΗ what is AH for this reaction? X(s) +02(g) + CO,(g) XC0,() AH = -1386.0 kJ terms of use privacy policy about us contact us help careers a 23
Make a non-spontaneous process spontaneous A process that is nonspontaneous can be made spontaneous by coupling it with another process tha is highly spontaneous. The coupling of nonspontaneous reactions with highly spontaneous ones is important in biological system. The oxidization of glucose, for example, is highly spontaneous: C6H12O6(s) + 60₂(g) → 6 CO₂(g) + 6 H₂O(1) Spontaneous reactions such as this ultimately drive the nonspontaneous reactions necessary to sustain life. Can you use Gibbs free energy, enthalpy, and entropy to argue this reaction is highly spontaneous?
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When a neutralization reaction was carried out using 100.0 mL of 0.7890M NH3 water and 100.0 mL of 0.7940M acetic acid, ΔT was found to be 4.76 °C. The specific heat of the reaction mixture was 4.104 J g-l K-1 and its density was 1.03 g mL-1. The calorimeter constant was 3.36 JK-1 a) Calculate ΔH neutralization for the reaction of NH3 and acetic acid. b) At the end of the experiment, it was discovered that the thermometer had not been calibrated. When it was calibrated, it was found that the thermometer read 0.50 °C low. What effect would this thermometer reading have on the reported DH neutralization calculated above? c) When the temperature-time data graph was reviewed, it was found that an error had been made in determining ΔT. Instead of 4.76 °C, ΔT was actually 4.70 °C. Based on this change only, calculate the correct ΔH neutralization for the reaction of NH3, and acetic acid. d) Calculate the percent error for the correct ΔH neutralization if aΔ DT of 4.76 °C had been used.…