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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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 = −…
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