Suppose a 500. mL flask is filled with 1.2 mol of N2 and 0.20 mol of O2. The following reaction becomes possible: N2(g) + O2(8)2NO(g) The equilibrium constant K for this reaction is 8.71 at the temperature of the flask. Calculate the equilibrium molarity of N₂. Round your answer to two decimal places. M × 5

Suppose a 500. mL flask is filled with 1.2 mol of N2 and 0.20 mol of O2. The following reaction becomes possible: N2(g) + O2(8)2NO(g) The equilibrium constant K for this reaction is 8.71 at the temperature of the flask. Calculate the equilibrium molarity of N₂. Round your answer to two decimal places. M × 5

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 14.36QE: Consider the system 4NH3(g)+3O2(g)2N2(g)+6H2O(l)H=1530.4kJ (a) How will the concentration of ammonia...

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