mixture of 0.856 mol of NO, 0.656 mol of H₂, and 1.16 mol of H₂O is placed in a 1.0-L vessel at 300 K. The following equilibrium is established: NO(g) + 2H₂(g) = N2(g) + 2H₂O(g) At equilibrium [NO] = 0.248 M. Part B Calculate the equilibrium concentration of N₂. Express the molarity to three decimal places. VE ΑΣΦ Submit Part C Calculate the equilibrium concentration of H₂O. Express the molarity to three decimal places. [5] ΑΣΦ Submit Request Answer Part D Request Answer Calculate Ke Express your answer to two significant figures. ? ? M M
mixture of 0.856 mol of NO, 0.656 mol of H₂, and 1.16 mol of H₂O is placed in a 1.0-L vessel at 300 K. The following equilibrium is established: NO(g) + 2H₂(g) = N2(g) + 2H₂O(g) At equilibrium [NO] = 0.248 M. Part B Calculate the equilibrium concentration of N₂. Express the molarity to three decimal places. VE ΑΣΦ Submit Part C Calculate the equilibrium concentration of H₂O. Express the molarity to three decimal places. [5] ΑΣΦ Submit Request Answer Part D Request Answer Calculate Ke Express your answer to two significant figures. ? ? M M
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 14.40QE
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