A 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: 2NO(g) + 2H₂(g) = N₂(g) + 2H₂O(g) At equilibrium [NO] = 0.248 M. ▼ Part C Calculate the equilibrium concentration of H₂O. Express the molarity to three decimal places. 15. ΑΣΦ 0.608 Submit Previous Answers Request Answer Part D ESS Ne X Incorrect; Try Again; 5 attempts remaining Calculate Ke Express your answer to two significant figures. IVE ΑΣΦ Kc = 7.9.10² ? ? M

A 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: 2NO(g) + 2H₂(g) = N₂(g) + 2H₂O(g) At equilibrium [NO] = 0.248 M. ▼ Part C Calculate the equilibrium concentration of H₂O. Express the molarity to three decimal places. 15. ΑΣΦ 0.608 Submit Previous Answers Request Answer Part D ESS Ne X Incorrect; Try Again; 5 attempts remaining Calculate Ke Express your answer to two significant figures. IVE ΑΣΦ Kc = 7.9.10² ? ? M

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 61QRT

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Question

The equilibrium concentrate of H2: 0.048 M The equilibrium concentrate of N2: 0.304M

U
A 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:
2NO(g) + 2H₂(g) = N₂(g) + 2H₂O(g)
At equilibrium [NO] = 0.248 M.
na
▼
Part C
Calculate the equilibrium concentration of H₂O.
Express the molarity to three decimal places.
195| ΑΣΦ
0.608
Submit Previous Answers Request Answer
X Incorrect; Try Again; 5 attempts remaining
Part D
Calculate Ke
Express your answer to two significant figures.
—| ΑΣΦ
Ke= 7.9.10²
Submit
Previous Answers Request Answer
?
X Incorrect; Try Again; 5 attempts remaining
?
M

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