Question 6Calculate the AG for the following process at 100 K and 300 K. Use thethermodynamic data from Appendix G in OpenStax Chemistry, 2e. If oneexists, calculate the temperature (in K) at which the process switchesbetween spontaneous and non-spontaneous.ZaCl()Zn (aq) + 2 Cl (ag)Report G to the tenths place.AGT="KபP

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Answered: Question 6 Calculate the AG for the…

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 combustion of acetylene is used in welder's torches because it produces a very hot flame: 5 C₂ H2(g) + O2(g) → 2 CO₂ (g) + H₂O(g) AH = -1255.5 kJ Substance Sº (J mol-¹ K-¹) C₂ H₂(g) 200.8 O₂(g) CO₂(g) H₂O(g) 205.0 213.6 188.7
a. Calculate Ecell and AG° (in kJ) and determine if the reaction is spontaneous. b. Calculate the equilibrium constant, K, at 298 K for the reaction using AG° = -RT In K. 4 Ag(s) + O2(g) + 4 H*(aq) → 4 Ag*(aq) + 2 H,O(1) O2(g) + 4 H*(aq) + 4 e +1.23 2 H2O(1) - +1.06 Br2(1) + 2 e 2 Br (aq) NO, (aq) + 4 H*(aq) + 3 e¯ Ag*(aq) + e - → NO(g) + 2 H,O(I) +0.96 +0.80 Ag(s) Do the signs/values of AG° and K make sense for this reaction given the cell potential?
3.65 g of zinc metal react according tyo the following reaction at 25 C. Is this reaction spontaneous? Zn (0 + 2H^+ (aq) -> zn^2= (aq) + H2 (g)
Here again is the balanced equation for the formation of hydrogen gas (H2(g)) that took place in the test tube when Zn(s) and HCl(aq) were combined: 2 HCl(aq) + Zn(s)--> H2(g) + ZnCl2(aq) This enthalpy and entropy values for this reaction are Δ H = − 80.7 k J and Δ S = 0.0140 k J K. If you perform this reaction at 25.0 degrees Celsius, what is the free energy change (in kJ) for this reaction? Round your answer to three significant figures
Determine the temperature of a reaction if K = 1.20 x 106 when AG° = +22.70 kJ/mol.
The overall reaction for the corrosion of iron (rusting) by oxygen is 4Fe(s) + 3O2 --> 2Fe2O3 (s) b. Calculate the equilibrium constant using ΔGo = -RT ln K.
Determine the equilibrium constant for a reaction at 200 K if AG =26.2 kJ/mol. (R = 8.314 J/mol · K)
14
Under the conditions shown below for the following reaction. Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g) AG° = -28.0 kJ P(CO) = 4.2 atm, P(CO2) = 1.8 atm Calculate AGrxn at 298 K, and indicate if the reaction is more or less spontaneous under these conditions than under standard conditions?
For the reaction A(aq) ---> B(aq) the variation in the standard free enthalpy is 3.50 kJ at 25 oC and 4.64 kJ at 45 oC. Calculate the value of the equilibrium constant for this reaction at 75°C.
Calculate AG° at 298 K for the reaction CS,1) + 3 0,(g) → CO,(g) + 2 SO,(g) CO,(g) + 2 SO, (g) > based on these reactions. C(s) + O,(g) → CO, (g) AG° = -397.28 kJ/mol S(s) + 0,(g) –→ SO, (g) AG° = -300.19 kJ/mol C(s) + 2 S(s) · CS,(1) AG° = +62.37 kJ/mol AG° = kJ/mol

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