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The equilibrium constant K-4.00 10-4 at the temperature of 500 ° C for the reaction 2HCN(g) * H2(g) + C2N2(g) Set up the equilibrium expression for the reaction. In an empty container of 12.00/1.00 mol of HCN (g), 2.00 mol of H2 (g) and 3.00 mol of C2N2 (g) were introduced. Is the system in equilibrium? If not, in what direction will the reaction go to achieve equilibrium?

The equilibrium constant K-4.00 10-4 at the temperature of 500 ° C for the reaction 2HCN(g) * H2(g) + C2N2(g) Set up the equilibrium expression for the reaction. In an empty container of 12.00/1.00 mol of HCN (g), 2.00 mol of H2 (g) and 3.00 mol of C2N2 (g) were introduced. Is the system in equilibrium? If not, in what direction will the reaction go to achieve equilibrium?

Chemistry
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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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The equilibrium constant K-4.00 10-4 at the temperature of 500 ° C for the reaction 2HCN(g) * H2(g) + C2N2(g) Set up the equilibrium expression for the reaction. In an empty container of 12.00/1.00 mol of HCN (g), 2.00 mol of H2 (g) and 3.00 mol of C2N2 (g) were introduced. Is the system in equilibrium? If not, in what direction will the reaction go to achieve equilibrium?
Transcribed Image Text:The equilibrium constant K-4.00 10-4 at the temperature of 500 ° C for the reaction 2HCN(g) * H2(g) + C2N2(g) Set up the equilibrium expression for the reaction. In an empty container of 12.00/1.00 mol of HCN (g), 2.00 mol of H2 (g) and 3.00 mol of C2N2 (g) were introduced. Is the system in equilibrium? If not, in what direction will the reaction go to achieve equilibrium?
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