2) Using ∆Gf^0 values, calculate Kp at 298 K for the reaction 2 NO2(g) N2O4(g) ∆Gf^0 = -4.73 kJ/mol For this reaction, determine the following: a. Effect of decrease in pressure in the number of moles of NO2. b. Equilibrium constant at 500 K. c. Effect of adding Ar gas on the number of moles of NO2.
2) Using ∆Gf^0 values, calculate Kp at 298 K for the reaction 2 NO2(g) N2O4(g) ∆Gf^0 = -4.73 kJ/mol For this reaction, determine the following: a. Effect of decrease in pressure in the number of moles of NO2. b. Equilibrium constant at 500 K. c. Effect of adding Ar gas on the number of moles of NO2.
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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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2) Using ∆Gf^0
values, calculate Kp at 298 K for the reaction
2 NO2(g) N2O4(g)
∆Gf^0 = -4.73 kJ/mol
For this reaction, determine the following:
a. Effect of decrease in pressure in the number of moles of NO2.
b. Equilibrium constant at 500 K.
c. Effect of adding Ar gas on the number of moles of NO2.
d. Temperature at which number of moles of NO2 and N2O4 are equal.
(Hint: calculate Kp first)
*Answer both items and final answers in 4 decimals
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