3) Calculate the standard Gibbs energy of the following reaction at 298 K:CH₂COOH (1)→ CO (g) + CH3OH (1)Hint: First, calculate the standard reaction enthalpy AH and the standard reaction entropyAS using standard entropies and enthalpies of formation of compounds in the Data Section.Then, calculate the standard Gibbs energy of this reaction.Cadmium (Continued)Cdo(s)CaCO,(s)Caesium (cesium)Cs(s)Cs(g)Cs' (aq)CalciumCa(s)Ca(g)Ca (aq)CIO(8)CaCO,(s) (calcite)CaCO,(s) (aragonite)CaF₂(s)CaCl₂(8)CaBry(s)M/(g mol-¹)C₂(g)CO(g)CO₂(g)128.40172.41132.91132.91132.9140.0840.0840.0856.08100.09100.0978.08110,99199.90AH/(kl mol-¹)-258.2-750.60+76.06-258.280+178.2-542.83-635.09-1206.9-1207.1-1219.6-795.8-682.80+1.895+716.68+831.90-110.53-393.51413 onCarbon (for 'organic' compounds of carbon, see Table 2.5)C(s) (graphite)12.011C(s) (diamond)12.011C(g)12.01124.02228.01144,01014010AGKJ mol¹)-228.4-669 A0+49.12-292.020+1443-553.58-604.03-1128.8-1127.8-1167.3-748,1-663.60+2.900+671.26+775.89-394.36105 00$20K molt54.892.585.23175.60+133.0541.42154.88-53.139.7592.988.768.87104.61305.7402.377158.10199.42197.67213.741176CK¹mot')43.4332.1720.79-10.525.3120.78642.8081.8881.2567.0372.598.5276.11320.83843.2129.1437.11

Answered: Image /qna-images/answer/5a0216d8-fab3-4bb9-996d-ffee2cc13bf5.jpg

3) Calculate the standard Gibbs energy of the following reaction at 298 K: CH₂COOH (1)→ CO (g) + CH₂OH (1) Hint: First, calculate the standard reaction enthalpy A,H and the standard reaction entropy AS using standard entropies and enthalpies of formation of compounds in the Data Section. Then, calculate the standard Gibbs energy of this reaction.

3) Calculate the standard Gibbs energy of the following reaction at 298 K: CH₂COOH (1)→ CO (g) + CH₂OH (1) Hint: First, calculate the standard reaction enthalpy A,H and the standard reaction entropy AS using standard entropies and enthalpies of formation of compounds in the Data Section. Then, calculate the standard Gibbs energy of this reaction.

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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(16) Solid potassium chlorate decomposes into solid potassium chloride and oxygen according to the following balanced chemical equation: KCIO, (s) → KCI (s) + 3/2 O, (g) Given the enthalpy of reaction is -77.6 kl and the entropy of reaction is 494.6 3/K, the overall Gibbs free energy change for this reaction at 40.0°C is: (A) (B) (C) (D) (E) -252 k -157 kJ -1.55 x 10 kJ -232.5 kJ -97.4 kJ
Solve correctly please.
(d) For the reaction: H3C. H3C. C-OH Cc=CH2 H3C H20 H,C H3C Reaction 2 Reaction 2 does not go to completion and the position of the reaction can be defined in terms of the equilibrium constant, K. (i) For the above reaction at 298K under specific conditions the following thermodynamic information were obtained, reaction Gibbs free energy (AreactG = -5.4 kJ mol-1), standard reaction enthalpy (AreactH® = -52.7 kJ mol-1) and standard reaction entropy (AreactS® = -0.16 kJ mol-1). From the above detail, calculate the equilibrium constant. (ii) Sketch a diagram of the Gibbs free energy versus reaction progress and on diagram label the reaction Gibbs free energy (A,react G) and standard reaction Gibbs free energy (Areact G®).
Use the data from this table of thermodynamic properties to calculate the maximum amount of work that can be obtained from the combustion of 1.00 mole of ethane, CH3CH3(g), at 25 °C and standard conditions. mo
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 26.0 °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. N₂(g) + 3H₂(g) → 2NH₂(g) P₁(s) + 20HF (g) 4PF, (g) + 10H₂(g) ΔΗ = -92. kJ AS = AG = | KJ -294. ΔΗ Which is spontaneous? this reaction the reverse reaction neither AS = = - 1005. kJ…
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 69.0 °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. HCH, CO₂(1)→ CH₂OH(g) + CO(g) Al₂O₂ (s) + 2Fe(s) -> 2A1(s) + Fe₂O₂ (s) AH = 172. kJ AS = 543. AG = Which is spontaneous? O this reaction O the reverse reaction Oneither ΔΗ = 852. 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
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.
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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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 87.0 °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. Al₂O3(s) + 2Fe(s) → 2Al(s) + Fe₂O₂ (s) AH = 852. kJ AS = 2272. AG = | KJ J K Which is spontaneous? this reaction the reverse reaction neither 3
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 24.0 °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. AH = 188. kJ AS = X Ś ? N₂H₂(g) + H₂(g) → 2NH₂(g) AG = 4 2 P₂(g) + 6Cl₂ (g) 4PC1₂ (g) 688. kJ Which is spontaneous? this reaction the reverse reaction neither AH = - 1207. kJ J AS =…