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)
Chemistry by OpenStax (2015-05-04)
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Chapter13: Fundamental Equilibrium Concepts
Section: Chapter Questions
Problem 12E: Show that the complete chemical equation, the total ionic equation, and the net ionic equation for...
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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)
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
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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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