Nitrosyl bromide decomposes according to the following equation: 2NOBr(g) -><- 2

Question

Nitrosyl bromide decomposes according to the following equation: 2NOBr(g) -><- 2NO(g) + Br2(g). A .84 mol sample of NOBr was placed in an empty 1.00L flask and then covered. At equilibrium, the flask contained .56 mol NOBr.

1. What are the concentrations of NO and Br2 in the flask at equilibrium?

2. Calculate the Kc for the reaction.

3.Explain what would happen to the above reaction if a catalyst was added

I really just need number 1 and 3 because then I can change moles into M for number 2 and plug them into the equation.

Explanation / Answer

1)moles of NO=0.84-0.56

=0.28

moles of Br2=0.28/2

=0.14

[NO]=0.28

[Br2]=0.14

2)Kc=[NO]^2[Br2]/[NOBr]^2

=0.035

3)if a catalyst were added only the speed of the reaction and not affect the Kc of the reaction

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