At 100.0°C, K. = 0.135 for the reaction 3H2(g) - N2(s) = 2NH3(g) Inareaction mixture at equilibrium at this temperature [NH3] = 0.00600 Mand [N2] = 4.01 M. (a) What are the partial pressures of all the gases in the mixture? PNH, = atm atm PN. = atm eTextbook and Media (b) Calculate Ka using the partial pressures. Enter your answer in scientific notation. K = x 10 (c) Calculate K, using the equation K, = K-(RT)ane_ Enter your answer in scientific notation. х 10

At 100.0°C, K. = 0.135 for the reaction 3H2(g) - N2(s) = 2NH3(g) Inareaction mixture at equilibrium at this temperature [NH3] = 0.00600 Mand [N2] = 4.01 M. (a) What are the partial pressures of all the gases in the mixture? PNH, = atm atm PN. = atm eTextbook and Media (b) Calculate Ka using the partial pressures. Enter your answer in scientific notation. K = x 10 (c) Calculate K, using the equation K, = K-(RT)ane_ Enter your answer in scientific notation. х 10

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 51P

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Methanol can be synthesized by means of the equilibriumreaction CO(g)+2H2(g)CH3OH(g) for which the equilibrium constant at 225°C is 6.08103. Assume that the ratio of the pressures of CO(g) and H2(g) is 1:2. What values should they have if the partial pressureof methanol is to be 0.500 atm?
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