At 100.0 °C, K. = 0.135 for the reaction3H2(3) + N2(g) = 2NH3(g)Ina reaction mixture at equilibrium at this temperature [NH3] = 0.0080O M and [N3] = 3.01 M.(a) What are the partial pressures of all the gases in the mixture?PNH,atmPi%3DatmPNaatm(b) Calculate K, using the partial pressures.Enter your answer in scientific notation.x 10(c) Calculate K, using the equationAngK, = Ke(RT)ª" .Enter your answer in scientific notation.x 10 i

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At 100.0 °C, K = 0.135 for the reaction 3H2(g) + N2(3) = 2NH3(9) In a reaction mixture at equilibrium at this temperature [NH3] = 0.0080O M and [N2) = 3.01 M. (a) What are the partial pressures of all the gases in the mixture? PNH, = atm P atm PN atm (b) Calculate K, using the partial pressures. Enter your answer in scientific notation. x 10 i (c) Calculate K, using the equation K, = K.(RT)ar. Enter your answer in scientific notation. x 10

At 100.0 °C, K = 0.135 for the reaction 3H2(g) + N2(3) = 2NH3(9) In a reaction mixture at equilibrium at this temperature [NH3] = 0.0080O M and [N2) = 3.01 M. (a) What are the partial pressures of all the gases in the mixture? PNH, = atm P atm PN atm (b) Calculate K, using the partial pressures. Enter your answer in scientific notation. x 10 i (c) Calculate K, using the equation K, = K.(RT)ar. Enter your answer in scientific notation. x 10

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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