Where possible, classify these systems as reactant-favored or product-favored at 298 K. If the direction cannot be determined from the information given, classify the reaction as "Insufficient information." Reactant-favored Product-favored Insufficient information 2 A(g)+B(s) = 3 C(g) 2 A(g) + 3 B(g) = 4 C(g) AH' = -193 kJ AH = -95 kJ 2 A(g)+B(g) = 4 C(g) A(s) + 2 B(g) = C(g) AH' = +322 kJ AH = +271 kJ %3D

Where possible, classify these systems as reactant-favored or product-favored at 298 K. If the direction cannot be determined from the information given, classify the reaction as "Insufficient information." Reactant-favored Product-favored Insufficient information 2 A(g)+B(s) = 3 C(g) 2 A(g) + 3 B(g) = 4 C(g) AH' = -193 kJ AH = -95 kJ 2 A(g)+B(g) = 4 C(g) A(s) + 2 B(g) = C(g) AH' = +322 kJ AH = +271 kJ %3D

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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N2(8) +0,(8) → 2NO (8 ) AH = 180.5 kJ NO (8) + -0,(8)→NO,(8) AH = -57.1 kJ Calculate the AHXN for the following reaction: N,+0,-NO,(8) 2
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 105.0 °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.
Consider the reaction 2NO2 (9) = N204(9) For each of the following mixtures of reactants and products at 25°C, predict the direction in which the reaction will shift to reach equilibrium. AG F(NO:(9)) = 52 kJ/mol AGN0.(0)) = 98 kJ/mol PNO, = PN,0, = 1.0 atm a. PNo, = 0.21 atm, PN,o, = 0.50 atm b. PNO2 0.21 atm, PN,04 0.84 atm с.
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1. Using Hess's Law, calculate AH for this reaction: (T: 4) 2H3BO3(aq) →→→ B₂O3(s) + 3H₂O(l) (1) H₂BO3(aq) → HBO₂(aq) + H₂O(E) AH = -0.020 kJ (2) 2B₂O3(s) + H₂O(l) → H₂B4O7(s) AH = -17.5 kJ (3) H₂B4O7(s) + H₂O(l) → 4HBO₂(aq) AH = -11.3 kJ
Calculate AH for the reaction 4 NH3 (g) + 5 02 (g) à 4 NO (g) + 6 H2O (g), from the following data N2 (g) + 02 (g) -> 2 NO (g) Ne (g) + 3 H2 (9) -> 2 NH3 (g) 2 H2 (9) ?H = -120.0 kJ ?H = -90.0 kJ + O2 (g) -> 2 H20 (g) ?H = -400.0 kJ Select one: O a. -1620 kJ/mol O b. -1260 kJ/mol O c. -430 kJ/mol O d. -860 kJ/mol
From the enthalpies of reaction 2C(s) + O2 (9) → 2C0(g) 2C(s) + O2 (9) + 4H2 (g) → 2CH3 OH(g) AH ΔΗ :-221.0kJ %3| :-402.4kJ calculate AH for the reaction CO(g) + 2H2 (g) → CH3 OH(g) Express your answer to three significant figures with the appropriate units.
Calculate AGºrxn for the reaction: BaCO3(s)→BaO(s)+CO₂(g) Use the following reactions and given AGºrxn values: Ba(s)+CO₂(g)+1/2O2(g) →BaCO3(s) AG°rxn=-1134.4kJ 2Ba(s)+O₂(g)→2BaO(s), AGºrxn=-520.3kJ BaCO3(s)→BaO(s)+CO₂(g). AGºrxn =
7. Calculate the standard enthalpy change at 25°C for the reaction CH, (g) + 2 H₂S (g) →→ CS₂ (1) + 4H₂(g) The values of AH'at 298 K for reactants and products are: Adf 298/kJ mol¹: CH4(g) = -74.8; H₂S (g)=-20.6; CS₂ (1)=+89.7; H₂(g) - 0.
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Question 18 of 25 > Given the reactions, X(s) + 0,(g) –→ XO(s) AH = -562.9 kJ XCO,(s) XO(s) + CO, (g) AH = +447.1 kJ what is AH for this reaction? X(S) + 글0(g) + CO,(g) XCO,(s) ΔΗ- kJ
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