Consider the reaction: N2O4 (g) ⟷ 2 NO2 (g) KP = 0.36 (at 100°C) The reaction above is carried out at the same temperature but the vessel contains only the reactant, PN2O4 = 0.0550 atm and none of the product. Complete an ICE diagram to find the equilibrium partial pressures for N2O4 and NO2.
Consider the reaction: N2O4 (g) ⟷ 2 NO2 (g) KP = 0.36 (at 100°C) The reaction above is carried out at the same temperature but the vessel contains only the reactant, PN2O4 = 0.0550 atm and none of the product. Complete an ICE diagram to find the equilibrium partial pressures for N2O4 and NO2.
Chemistry
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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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Consider the reaction:
N2O4 (g) ⟷ 2 NO2 (g) KP = 0.36 (at 100°C)
The reaction above is carried out at the same temperature but the vessel contains only the reactant, PN2O4
= 0.0550
atm and none of the product. Complete an ICE diagram to find the equilibrium partial pressures for N2O4 and NO2.
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