The equilibrium constant for the reaction 2NO(g)+Br2(g)⥫⥬2NOBr(g) is Kc=1.3×10−2 at 1000 K. At this temperature does the equilibrium favor NO and Br2, or does it favor NOBr?
Calculate Kc for 2NOBr(g)⥫⥬2NO(g)+Br2(g).

Question

The equilibrium constant for the reaction 2NO(g)+Br2(g)⥫⥬2NOBr(g) is Kc=1.3×10−2 at 1000 K. At this temperature does the equilibrium favor NO and Br2, or does it favor NOBr?
Calculate Kc for 2NOBr(g)⥫⥬2NO(g)+Br2(g).

The equilibrium constant for the reaction 2NO(g)+Br2(g)⥫⥬2NOBr(g) is Kc=1.3×10−2 at 1000 K. At this temperature does the equilibrium favor NO and Br2, or does it favor NOBr?

Calculate Kc for 2NOBr(g)⥫⥬2NO(g)+Br2(g).

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The equilibrium constant for the reaction 2NO(g)+Br2(g)⥫⥬2NOBr(g) is Kc=1.3×10−2 at 1000 K. At this temperature does the equilibrium favor NO and Br2, or does it favor NOBr? Calculate Kc for 2NOBr(g)⥫⥬2NO(g)+Br2(g).

Unlock all answers

Related textbook solutions

Basic Chemistry

Principles of Chemistry Molecular Approach

Chemistry: Structure and Properties

Principles of Chemistry Molecular Approach

Chemistry: A Molecular Approach

Chemistry: A Molecular Approach

Principles of Chemistry: A Molecular Approach

Chemistry: The Central Science

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The equilibrium constant for the reaction 2NO(g)+Br2(g)⥫⥬2NOBr(g) is Kc=1.3×10−2 at 1000 K. At this temperature does the equilibrium favor NO and Br2, or does it favor NOBr?

Calculate Kc for 2NOBr(g)⥫⥬2NO(g)+Br2(g).