Consider the following equilibrium: 2 NO(g) + Br2(g) ⇌ 2 NOBr(g). 0.60 mol of NOBr(g) was placed in a rigid 1.00 L flask containing no NO(g) or Br2(g) at room temperature. At equilibrium the flask contained 0.30 mol of NOBr(g) and 0.30 mol NO(g). Calculate the equilibrium constant Kc for this reaction. Correct! 6.67 0.167 3.33 0.333
Consider the following equilibrium: 2 NO(g) + Br2(g) ⇌ 2 NOBr(g). 0.60 mol of NOBr(g) was placed in a rigid 1.00 L flask containing no NO(g) or Br2(g) at room temperature. At equilibrium the flask contained 0.30 mol of NOBr(g) and 0.30 mol NO(g). Calculate the equilibrium constant Kc for this reaction. Correct! 6.67 0.167 3.33 0.333
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter19: The Chemistry Of The Main-group Elements
Section: Chapter Questions
Problem 60QRT
Related questions
Question
Consider the following equilibrium: 2 NO(g) + Br2(g) ⇌ 2 NOBr(g).
0.60 mol of NOBr(g) was placed in a rigid 1.00 L flask containing no NO(g) or Br2(g) at room temperature. At equilibrium the flask contained 0.30 mol of NOBr(g) and 0.30 mol NO(g).
Calculate the equilibrium constant Kc for this reaction.
Correct!
6.67
0.167
3.33
0.333
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