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Consider the equilibrium system described by the chemical reaction below. The decomposition of NOBR has a value Kc equal to 3.07 x 10-4 at 297 K. If an initial solution of 0.20 M NOBR decomposes, what will the concentration of NO be at equilibrium? 2 NOBR(g) =2 NO(g) + Br2(g) 1 2 3 Based on the given values, set up ICE table in order to determine the unknown. 2 NOBr(g) = 2 NO(g) + Br2(g) Initial (M) Change (M) Equilibrium (M)

Consider the equilibrium system described by the chemical reaction below. The decomposition of NOBR has a value Kc equal to 3.07 x 10-4 at 297 K. If an initial solution of 0.20 M NOBR decomposes, what will the concentration of NO be at equilibrium? 2 NOBR(g) =2 NO(g) + Br2(g) 1 2 3 Based on the given values, set up ICE table in order to determine the unknown. 2 NOBr(g) = 2 NO(g) + Br2(g) Initial (M) Change (M) Equilibrium (M)

General, Organic, and Biological Chemistry
General, Organic, and Biological Chemistry
7th Edition
ISBN:9781285853918
Author:H. Stephen Stoker
Publisher:H. Stephen Stoker
Chapter9: Chemical Reactions
Section: Chapter Questions
Problem 9.84EP: Based on the diagrams, chemical reaction, and reaction conditions depicted in Problem 9-83, which of...
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8:02 Question 4 of 8 Submit Consider the equilibrium system described by the chemical reaction below. The decomposition of NOBR has a value Kc equal to 3.07 x 10-4 at 297 K. If an initial solution of 0.20 M NOBR decomposes, what will the concentration of NO be at equilibrium? 2 NOBr(g) = 2 NO(g) + Br2(g) 1 2 3 Based on the given values, set up ICE table in order to determine the unknown. 2 NOBR(g) = 2 NO(g) Br2(g) + Initial (M) Change (M) Equilibrium (M) 5 RESET 0.20 0.40 +x +x2 +2x +2x? -x -2x -2x² 0.20 - x 0.20 + x 0.40 - x 0.40 + x 0.20 - 2x 0.20 + 2x 0.40 - 2x 0.40 + 2x Tap here or pull up for additional resources
Transcribed Image Text:8:02 Question 4 of 8 Submit Consider the equilibrium system described by the chemical reaction below. The decomposition of NOBR has a value Kc equal to 3.07 x 10-4 at 297 K. If an initial solution of 0.20 M NOBR decomposes, what will the concentration of NO be at equilibrium? 2 NOBr(g) = 2 NO(g) + Br2(g) 1 2 3 Based on the given values, set up ICE table in order to determine the unknown. 2 NOBR(g) = 2 NO(g) Br2(g) + Initial (M) Change (M) Equilibrium (M) 5 RESET 0.20 0.40 +x +x2 +2x +2x? -x -2x -2x² 0.20 - x 0.20 + x 0.40 - x 0.40 + x 0.20 - 2x 0.20 + 2x 0.40 - 2x 0.40 + 2x Tap here or pull up for additional resources
Expert Solution
Step 1

For the given below reaction:

2 NOBr (g)⇌ 2 NO(g)  + Br2(g)

The ICE table has to be set up to determine the unknown.

Given :

The initial concentration of NOBr is 0.2 M.

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