Reaction at 25.0oC CO(g) + NO(g) → CO2(g) + N2(g) starts with the following initial partial pressures: (PCO2)0 = 0.50 atm, (PN2)0= 0.60 atm, (PCO)0= 5.0×10–35 atm, and (PNO)0 = 5.×10-36 atm. Substance ∆Gof, kJ mol CO2(g) – 394.4 N2(g) 0 CO(g) – 137.3 NO(g) + 86.7 Use the attached standard Gibbs free energies of formation to calculate: (a) KP for the reaction, (b) the immediate Gibbs free energy change for the reaction, ∆Grxn, and (c) check the correct box predicting the direction in which reaction proceeds. Enter your answers with correct units and significant figures, and check the correct box below: Reaction proceeds spontaneously forward towards equilibrium. Reaction is at equilibrium. Reaction proceeds spontaneously backward towards equilibrium.
Reaction at 25.0oC CO(g) + NO(g) → CO2(g) + N2(g) starts with the following initial partial pressures: (PCO2)0 = 0.50 atm, (PN2)0= 0.60 atm, (PCO)0= 5.0×10–35 atm, and (PNO)0 = 5.×10-36 atm. Substance ∆Gof, kJ mol CO2(g) – 394.4 N2(g) 0 CO(g) – 137.3 NO(g) + 86.7 Use the attached standard Gibbs free energies of formation to calculate: (a) KP for the reaction, (b) the immediate Gibbs free energy change for the reaction, ∆Grxn, and (c) check the correct box predicting the direction in which reaction proceeds. Enter your answers with correct units and significant figures, and check the correct box below: Reaction proceeds spontaneously forward towards equilibrium. Reaction is at equilibrium. Reaction proceeds spontaneously backward towards equilibrium.
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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Reaction at 25.0oC
CO(g) + NO(g) → CO2(g) + N2(g)
starts with the following initial partial pressures:
(PCO2)0 = 0.50 atm, (PN2)0= 0.60 atm, (PCO)0= 5.0×10–35 atm, and (PNO)0 = 5.×10-36 atm.
|
Substance |
∆Gof, kJ mol |
|
CO2(g) |
– 394.4 |
|
N2(g) |
0 |
|
CO(g) |
– 137.3 |
|
NO(g) |
+ 86.7 |
Use the attached standard Gibbs free energies of formation to calculate: (a) KP for the reaction, (b) the immediate Gibbs free energy change for the reaction, ∆Grxn, and (c) check the correct box predicting the direction in which reaction proceeds. Enter your answers with correct units and significant figures, and check the correct box below:
Reaction proceeds spontaneously forward towards equilibrium.
Reaction is at equilibrium.
Reaction proceeds spontaneously backward towards equilibrium.
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