15 (b) Calculate K, using the partial pressures.Enter your answer in scientific notation.Kp =x 10(c) Calculate K, using the equation4ngKp = Ke(RT)ª": .Enter your answer in scientific notation.Kp =iх 10i At 100.0 °C, Kc = 0.135 for the reaction3H2(g) + N2(g) 2NH3(s)%3DIn a reaction mixture at equilibrium at this temperature [NH3] = 0.00600 M and [N2] = 7.01 M.(a) What are the partial pressures of all the gases in the mixture?PNH;iatm%3DatmPH2PN2atmeTextbook and Media

Answered: Image /qna-images/answer/3f0095a3-bcee-4f9a-a802-792f9540d41e.jpg

At 100.0 °C, K = 0.135 for the reaction %3D 3H2(g) + N2(g) 2NH3(3) In a reaction mixture at equilibrium at this temperature [NH3] = 0.00600 M and [N2] = 7.01 M. %3D (a) What are the partial pressures of all the gases in the mixture? PNH3 i atm %3D PH2 i atm %3D PN, = i atm

At 100.0 °C, K = 0.135 for the reaction %3D 3H2(g) + N2(g) 2NH3(3) In a reaction mixture at equilibrium at this temperature [NH3] = 0.00600 M and [N2] = 7.01 M. %3D (a) What are the partial pressures of all the gases in the mixture? PNH3 i atm %3D PH2 i atm %3D PN, = i atm

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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Question

(b) Calculate K, using the partial pressures.
Enter your answer in scientific notation.
Kp =
x 10
(c) Calculate K, using the equation
4ng
Kp = Ke(RT)ª": .
Enter your answer in scientific notation.
Kp =
i
х 10
i

At 100.0 °C, Kc = 0.135 for the reaction
3H2(g) + N2(g) 2NH3(s)
%3D
In a reaction mixture at equilibrium at this temperature [NH3] = 0.00600 M and [N2] = 7.01 M.
(a) What are the partial pressures of all the gases in the mixture?
PNH;
i
atm
%3D
atm
PH2
PN2
atm
eTextbook and Media

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