Answer the following questions about the reaction represented above at 298 K. B I U x² X₂ 3 (a) Using the information in the table above, calculate the value of AS for the reaction. B I U C S2 X² X₂ 3 2 NO(g) + O₂(g) → 2 NO₂(g) C E 4 S2 E NO(g) O₂(g) NO₂(9) (b) is the reaction thermodynamically favorable at 298 K? Justify your answer based on the calculation of the value and sign of AG*. AH = -112 kJ/mol Absolute Entropy at 298 K (J/(K mol)) 211 205 240 0/10000 Word Limit 10000 Word ℗ Submit Q

Answer the following questions about the reaction represented above at 298 K. B I U x² X₂ 3 (a) Using the information in the table above, calculate the value of AS for the reaction. B I U C S2 X² X₂ 3 2 NO(g) + O₂(g) → 2 NO₂(g) C E 4 S2 E NO(g) O₂(g) NO₂(9) (b) is the reaction thermodynamically favorable at 298 K? Justify your answer based on the calculation of the value and sign of AG*. AH = -112 kJ/mol Absolute Entropy at 298 K (J/(K mol)) 211 205 240 0/10000 Word Limit 10000 Word ℗ Submit Q

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 7.0 °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. AH = 76. kJ J AS = 308. K 2NOCI(g) → 2No(g) + Cl, (g) AG = ||kJ Which is spontaneous? this reaction the reverse reaction neither
Km.201.
Using the values provided in the table below, calculate ΔHr for the following reaction: 2CO2(g) + 4H2O(g) → 2CH3OH(l) + 3O2(g) a. -2158 kJ mol–1 b. 1354 kJ mol–1 c. -402 kJ mol–1 d. -435 kJ mol–1 e. -1354 kJ mol–1
Consider the following reaction; A(g) + B(g) → c(s) + D(g); AH = 159.1 kJ; AG = 164.1kJ at 298 K %3D The reaction is spontaneous at relatively high temperatures only The reaction is spontaneous at all temperatures The reaction is nonspontaneous at all temperatures. The reaction is at equilibrium at 298 K The reaction is spontaneous at relatively low temperatures only
18,19 plz
Use standard thermodynamic data to calculate G at 298.15 K for the following reaction, assuming that all gases have a pressure of 20.46 mm Hg.2NO(g) + O2(g)2NO2(g) G = ______kJ/mol
In which of the following reactions is ASº expected to be negative? O L(s)I(g) O 2NH;(g) → N(g) + 3H3(g) O 2H,0(g) → 2H,(g) + O>(g) O CH;OH(g) → CH;OH(I) O AS° is not expected to be negative for any of these.
1. Argon is allowed to expand isothermally (at 298 K) and reversibly from an initial molar volume of 5.0 L/mol to a final molar volume of 11 L/mol. (a) Calculate the work (in units of kJ to 4 sig. figs.) done assuming it behaves as an ideal gas (b) Calculate the work (in units of kJ to 4 sig. figs) assuming it is non-ideal using the van der Waals equation where a = 1.34 atm L2 mol-2 b = 3.20 x 10-2 L mol-1
Given the information below: 3M(g) = K.=6.88 × 10~3 27(g) 2Z(g) = 3Q(g)+6X(g) K,=3.12 × 102
2. For the following reaction at 25°C, AG° is -118.4 kJ. At what pressure of O2 gas does AG = 0 at 25°C? 2 KCIO3 (s) + 2 KCI (s) + 3 O2 (g)