For the following reaction, K = 2.7×108 at 300 K. 3 H2(g) + N2(g) = 2 NH3(g) In an experiment carried out at 300 K, the initial concentrations of H2(g) and N2(g) are each equal to 2.0 mol L -1 Which of the following statements about the equilibrium concentrations is correct? Note: In the statements below, << means "much less than". O [H2] = [N2]< [NH3] O [H2] << [N2]~ [NH3] O [H2] - [N2] = [NH3] O [N2] << [H2] < [NH3] O [NH3] << [N2] ~ [H2]

For the following reaction, K = 2.7×108 at 300 K. 3 H2(g) + N2(g) = 2 NH3(g) In an experiment carried out at 300 K, the initial concentrations of H2(g) and N2(g) are each equal to 2.0 mol L -1 Which of the following statements about the equilibrium concentrations is correct? Note: In the statements below, << means "much less than". O [H2] = [N2]< [NH3] O [H2] << [N2]~ [NH3] O [H2] - [N2] = [NH3] O [N2] << [H2] < [NH3] O [NH3] << [N2] ~ [H2]

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter12: Gaseous Chemical Equilibrium

Section: Chapter Questions

Problem 14QAP: Consider the following reaction at 1000 C: NO(g)+12 Cl2(g)NOCl(g) (a) Write an equilibrium constant...

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7-64 As we shall see in Chapter 20, there are two forms of glucose, designated alpha and betawhich are in equilibrium in aqueous solution. The equilibrium constant for the reaction is 1.5 at 30°C. (a) If you begin with a fresh 1.0 M solution of D-glucose in water, what will be its concentration when equilibrium is reached? (b) Calculate the percentage of glucose and of glucose present at equilibrium in aqueous solution at 30°C.
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