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17) concentrations were measured: [N2] = 3.0 x 10²M, [H2] = 3.7 x 10²M, [NH3] = 1.6 x 10²M. What is Kc? 2NH3(g) → N2(g) + 3H2(g) At 500 K, the following a) 0.0059 b) 168 c) 0.069 d) 215

17) concentrations were measured: [N2] = 3.0 x 10²M, [H2] = 3.7 x 10²M, [NH3] = 1.6 x 10²M. What is Kc? 2NH3(g) → N2(g) + 3H2(g) At 500 K, the following a) 0.0059 b) 168 c) 0.069 d) 215

Chemistry: An Atoms First Approach
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 111CP
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2NH3(g) → N2(g) + 3H2(g) At 500 K, the following 17) concentrations were measured: [N2] = 3.0 x 102M, [H2] = 3.7 x 10²M, [NH3] = 1.6 x 10²M. What is Kc? %3D %3D a) 0.0059 b) 168 c) 0.069 d) 215 18) If 2.00 moles of hydrogen and iodine are allowed to react in a10.0 L vessel according to the following reaction with Kc= 64.0 at a certain temperature, H2(g) + 12(g) <→2 HI(g), what will be the equilibrium concentration of HI? a) 0.16 M c) 0.48 M d) 0.64 M b) 0.32 M Type here to search
Transcribed Image Text:2NH3(g) → N2(g) + 3H2(g) At 500 K, the following 17) concentrations were measured: [N2] = 3.0 x 102M, [H2] = 3.7 x 10²M, [NH3] = 1.6 x 10²M. What is Kc? %3D %3D a) 0.0059 b) 168 c) 0.069 d) 215 18) If 2.00 moles of hydrogen and iodine are allowed to react in a10.0 L vessel according to the following reaction with Kc= 64.0 at a certain temperature, H2(g) + 12(g) <→2 HI(g), what will be the equilibrium concentration of HI? a) 0.16 M c) 0.48 M d) 0.64 M b) 0.32 M Type here to search
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