Directions: Given the AH° and AS°, Calculate the AG° values for the following reactions and indicate whether the reaction is spontaneous under standard conditions. AH° (kJ) AS° (J/K) 1. C (graphite) + 2H2 (g) → CH, (g) -74.9 +186 .3 2. CH, CH, (g) → H2 (g) + C2H4 (g) +137 +121 3. N2 (g) +2H2 (g) → N2H4 (I) +50.6 -331

Directions: Given the AH° and AS°, Calculate the AG° values for the following reactions and indicate whether the reaction is spontaneous under standard conditions. AH° (kJ) AS° (J/K) 1. C (graphite) + 2H2 (g) → CH, (g) -74.9 +186 .3 2. CH, CH, (g) → H2 (g) + C2H4 (g) +137 +121 3. N2 (g) +2H2 (g) → N2H4 (I) +50.6 -331

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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What is the lowest temperature at which the reaction is spontaneous under standard conditions? H2O (g) + C (s) -> H2 (g) + CO (g)
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Aa.46. We start with a pure sample of A(g). The following equilibrium is established: 2 A(g) <---> B(g) + C(g) The total pressure is 8.75 atm and the temperature is 25.0oC. The partial pressure of A(g) is 5.20 atm. Calculate the value of the standard Gibbs free enthalphy change (in kJ) for this reaction at 25.0oC.
Σ *00 For a particular reaction, AH = 81.95 kJ and AS = 27.0 J/K. Calculate AG for this reaction at 298 K. AG = %3D What can be said about the spontaneity of the reaction at 298 K? O The system is spontaneous in the reverse direction. O The system is at equilibrium. O The system is spontaneous as written. 8:12 PH (口四< 11/8/20 F5 F8 F12 PrtScr Insert Delete Backspace $4 % 8. 5. 7. 24 Alt Ctri
Determine AG° for the reaction 2 SO,(g) + 0,(g) →2 SO3(g) at 25 °C. Thermodynamic Data at 25 °C Species AH? in kJ/mol AG? in kJ/mol S° in J/(mol·K) O2 (g) SO2 (g) SO3 (g) 0. 205.0 -296.8 -300.1 248.2 -395.7 -371.1 256.8
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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?
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 63.0 °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.
Calculate the AH°, AS°, and AG° at 298 K for the following reaction: (Use the values found in Thermodynamic Properties to calculate your answers for questions a and b.) Al2O3(s) + 3 C(graphite) + 3 Cl₂(g) → 2 AICI 3(s) + 3 CO(g) 4.0 -64 a) ΔΗΟ kJ/mol b) AS° ✓ J/K.mol kJ/mol (Determine from the temperature, AH and AS) c) AGO 4.0 76.9 4.0 -89 (d) Is the reaction extensive at standard conditions and 298 K? O Yes O NO (e) Write the expression for K. (Format example: Kp = pHC12 / pH₂. pCl₂ would be entered as K_{p} = pHCI^{2}/pH_{2}. pCl_{2}.) Help chemPad XX (PCO)3 (pCl₂)³ ← Greek (PCO)^3/(pCl_2)^3 Your answer provides a different type of equation than was expected. (f) Calculate the value of K at 298 K 2.51e-16 X (Please answer to 3 significant figures.) (g) Estimate the value of K at 600 K. 1.79e-8 X (Please answer to 3 significant figures.)
One of the reactions that destroys ozone in the upper atmosphere is NO(g) + O3(g) ⇒ NO2 (g) + O2(g) Substance and State AGf (kJ/mol) NO(g) 87 NO₂(g) 52 0₂ (9) 0 03 (9) 163 a Calculate ΔG° (at 298 K) for this reaction. AG = -198 kJ b Calculate K (at 298 K) for this reaction. K =
On the basis of AG° for each of the following reac- tions, decide whether the reaction is spontaneous or nonspon- taneous as written. Or, if you expect an equilibrium mixture with significant amounts of both reactants and products, say 18.51 so. a. SO2(g) + 2H,S(g) → 3S(s) + 2H,O(g); AG° = –91 kJ b. 2H,O2(aq) O2(g) + 2H2O(I); AG° = -211 kJ