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For the unbalanced reaction H2​(g)+NO(g)<--->H2​O(g)+N2​(g) the initial concentrations are 6.75 M H2, 7.00 M NO, and no H2O or N2. At equilibrium, [N2] = 1.00  M. 1. Balance the equation using lowest-whole-number coefficients. Be sure to include states of matter in your equation. 2.Calculate the concentrations of H2, NO, and H2O at equilibrium.      ? M H2         ? M NO          ? M H2O    3. Calculate the value of K under the reaction conditions at equilibrium.

For the unbalanced reaction H2​(g)+NO(g)<--->H2​O(g)+N2​(g) the initial concentrations are 6.75 M H2, 7.00 M NO, and no H2O or N2. At equilibrium, [N2] = 1.00  M. 1. Balance the equation using lowest-whole-number coefficients. Be sure to include states of matter in your equation. 2.Calculate the concentrations of H2, NO, and H2O at equilibrium.      ? M H2         ? M NO          ? M H2O    3. Calculate the value of K under the reaction conditions at equilibrium.

Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter16: Spontaneity Of Reaction
Section: Chapter Questions
Problem 62QAP: Consider the reaction NH4+(aq) H+(aq)+NH3(aq) Use G f for NH3(aq) at 25C=26.7 kJ/mol and the...
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For the unbalanced reaction

H2​(g)+NO(g)<--->H2​O(g)+N2​(g)

the initial concentrations are 6.75 M H2, 7.00 M NO, and no H2O or N2. At equilibrium, [N2] = 1.00  M.

1. Balance the equation using lowest-whole-number coefficients. Be sure to include states of matter in your equation.

2.Calculate the concentrations of H2, NO, and H2O at equilibrium.
     ? M H2   
     ? M NO    
     ? M H2O   
3. Calculate the value of K under the reaction conditions at equilibrium.

 
 
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