The equilibrium constant Kc = 4.0 at a certain temperature. A reaction is carried out starting with 2.0 M of CO and 2.0 M H₂O(g). What will be the equilibrium concentration of H₂? CO(g) + H2O(g) → CO2 (g) + Hz (g) 14 a) 2.0 M b) 1.3 M c) 0.75 M d) 0.67 M e) 1.5 M ⇒ Consider the reaction: N2(g) + O2(g) 2NO(g), Ke=0.10 at 2000°C. Starting with initial concentrations of 0.040 mol/L of N₂ and 0.040 mol/L of O2, calculate the equilibrium concentration of NO, in mol/L. a) 5.4 x 10-3 M b) 0.0092 M c) 0.011 M d) 0.080 M e) 0.10 M f) 0.031 M g) 0.040 M h) 0.065 M

The equilibrium constant Kc = 4.0 at a certain temperature. A reaction is carried out starting with 2.0 M of CO and 2.0 M H₂O(g). What will be the equilibrium concentration of H₂? CO(g) + H2O(g) → CO2 (g) + Hz (g) 14 a) 2.0 M b) 1.3 M c) 0.75 M d) 0.67 M e) 1.5 M ⇒ Consider the reaction: N2(g) + O2(g) 2NO(g), Ke=0.10 at 2000°C. Starting with initial concentrations of 0.040 mol/L of N₂ and 0.040 mol/L of O2, calculate the equilibrium concentration of NO, in mol/L. a) 5.4 x 10-3 M b) 0.0092 M c) 0.011 M d) 0.080 M e) 0.10 M f) 0.031 M g) 0.040 M h) 0.065 M

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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