The equilibrium for the formation of dinitrogen tetraoxide gas (N,0.) from nitrogen dioxide (NO2) strongly favors reactants at ambient temperatures: 2 NO, (g) + N2O2 (g) What is the value of Kp at this same temperature? K = 1.7 x 1026 at 40,0°C (A) (B) (C) 4.4 x 10-25 6.6 x 1028 5.2 x 107 (D) 6.5 x 1030 (E) 5.9 x 1025

The equilibrium for the formation of dinitrogen tetraoxide gas (N,0.) from nitrogen dioxide (NO2) strongly favors reactants at ambient temperatures: 2 NO, (g) + N2O2 (g) What is the value of Kp at this same temperature? K = 1.7 x 1026 at 40,0°C (A) (B) (C) 4.4 x 10-25 6.6 x 1028 5.2 x 107 (D) 6.5 x 1030 (E) 5.9 x 1025

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 14.19QE: At 2000 K, experiments show that the equilibrium constant for the formation of water is 1.6 1010....

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Consider the equation G = G + RT ln(Q). What is the value of G for a reaction at equilibrium? What does Q equal at equilibrium? At equilibrium, the previous equation reduces to G = RT ln(K). When G 0, what does it indicate about K? When G 0, what does it indicate about K? When t G = 0, what does it indicate about K? G predicts spontaneity for a reaction, whereas G predicts the equilibrium position. Explain what this statement means. Under what conditions can you use G to determine the spontaneity of a reaction?
For the reaction C(s)+CO2(g)2CO(g) K=168 at 1273 K. If one starts with 0.3 atm of CO2 and 12.0 g of C at 1273 K, will the equilibrium mixture contain (a) mostly CO2? (b) mostly CO? (c) roughly equal amounts of CO2 and CO? (d) only C?
Consider the decomposition equilibrium for dinitrogen pentoxide: 2N2O5(g)4NO2(g)+O2(g) At a certain temperature and a total pressure of 1.00 atm, the N2O5 is 0.50% decomposed (by moles) at equilibrium. a. If the volume is increased by a factor of 10.0. will the mole percent of N2O5 decomposed at equilibrium be greater than, less than. or equal to 0.50%? Explain your answer. b. Calculate the mole percent of N2O5 that will be decomposed at equilibrium if the volume is increased by a factor of 10.0.
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The reaction, 3 H2(g) + N2(g) (g), has the fol lowing equilibrium constants at the temperatures given: atT=25°C,K= 2.8 X 104 at T = 500°C, A = 2.4 X IO"7 At which temperature are reactants favored? At which temperature are products favored? YVhat can you say about the reaction if the equilibrium constant is 1.2 at 127°C?
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For the system SO3(g)SO2(g)+12 O2(g)at 1000 K, K=0.45. Sulfur trioxide, originally at 1.00 atm pressure, partially dissociates to SO2 and O2 at 1000 K. What is its partial pressure at equilibrium?
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