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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The equilibrium constant of a system, K, can be related to the standard free energy change, AGO, using the following equation: AG-RT In K where I is a specified temperature in kelvins (usually 298 K) and R is equal to 8.314 J/(K.mol). Under conditions other than standard state, the following equation applies: AG = AG° + ᎡᏆ ln Q In this equation, Qis the reaction quotient and is defined the same manner as K except that the concentrations or pressures used are not necessarily the equilibrium values. Part A Acetylene, C₂ H2, can be converted to ethane, C₂H6, by a process known as hydrogenation. The reaction is C₂H₂(g) + 2H₂(g) = C₂H6(g) Given the following data at standard conditions (all pressures equal to 1 atm and the common reference temperature 298 K), what is the value of Kp for this reaction? 9A V—| ΑΣΦ Substance Express your answer using two significant figures. ►View Available Hint(s) t C₂ H₂(g) H₂(g) C₂H6(g) P ? Review | Constants | Periodic Table AG (kJ/mol) 209.2 0 -32.89
A critical reaction in the production of energy to do work or drive chemical reactions in biological systems is the hydrolysis of adenosine triphosphate, ATP, to adenosine diphosphate, ADP, as described by the reaction АТР(aq) + H,О() — ADP(aq) + HPO, (aq) for which AGan = -30.5 kJ/mol at 37.0 °C and pH 7.0. Calculate the value of AGxn in a biological cell in which [ATP] = 5.0 mM, [ADP] = 0.10 mM, and [HPO?-] = 5.0 mM. AGrxn = kJ/mol Is the hydrolysis of ATP spontaneous under these conditions? yes no
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
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.…
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Can some one explain the difference/ comments of equations and their si units
From the enthalpies of reaction 2C(s) + O2 (9) → 2C0(g) 2C(s) + O2 (9) + 4H2 (g) → 2CH3 OH(g) AH ΔΗ :-221.0kJ %3| :-402.4kJ calculate AH for the reaction CO(g) + 2H2 (g) → CH3 OH(g) Express your answer to three significant figures with the appropriate units.
A critical reaction in the production of energy to do work or drive chemical reactions in biological systems is the hydrolysis of adenosine triphosphate, ATP, to adenosine diphosphate, ADP, as described by the reaction ATP(aq) + H,O(1) → ADP(aq) + HPO (aq) for which AGixn = -30.5 kJ/mol at 37.0 °C and pH 7.0. Calculate the value of AGxn in a biological cell in which [ATP] = 5.0 mM, [ADP] = 0.40 mM, and [HPO?-] = 5.0 mM. AGxn kJ/mol %3D Is the hydrolysis of ATP spontaneous under these conditions? O yes
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?
(a) Calculate ΔH0rxn , ΔS0rxn and ΔG0rxn for the reaction A + 3B -> 2P under standard conditions (25oC), using the following data and comment on whether the reaction is spontaneous. Standard entropy of formation ΔSf°(A) = 191.6 J.mol-1.K-1 Standard entropy of formation ΔSf° (B) = 130.7 J.mol-1.K-1 Standard entropy of formation ΔSf° (P) = 192.8 J.mol-1.K-1 Standard enthalpy of formation ΔHf° (P) = −45.9 kJ.mol-1 A and B are elements whose enthalpies of formation = 0 (b) 0 moles of gas A and 1.0 moles of gas B are added to a 2-litre reactor which is then sealed. The reactor is maintained at a constant temperature of 25oC the following reaction occurs until equilibrium is reached: A + B ⇄ AB. At equilibrium, there are 0.75 moles of product AB in the reactor, which is also a gas. (i) Calculate the molarities of A, B and AB at equilibrium and the equilibrium constant Kc. (ii)…
Carbon dioxide dissolves in water to form carbonic acid. Estimate the thermodynamic equilibrium constant for this reaction using the AG; values in the table. Substance AG; (kJ/mol) H,CO, (aq) -616.1 H,O(1) -237.1 CO,(g) -394.4 K = Carbonic acid then ionizes in water (K = 4.5 x 10-7). Ignoring K2, estimate K for the overall process by which CO, and H,O form H* and HCO,. K = What is the pressure of CO, in equilibrium with carbonated water at 25 °C and pH = 4.78? Роо, atm