Respuesta :
Explanation:
[tex]2NO(g) + Br_2(g)\rightleftharpoons 2NOBr(g)[/tex]
Equilibrium constant of reaction = [tex]K=154[/tex]
Concentration of NO = [tex][NO]=\frac{2.69\times 10^{-2} mol}{1 L}=2.69\times 10^{-2} M[/tex]
Concentration of bromine gas = [tex][Br_2]=\frac{3.85\times 10^{-2} mol}{1 L}=3.85\times 10^{-2} M[/tex]
Concentration of NOBr gas = [tex][Br_2]=\frac{9.56\times 10^{-2} mol}{1 L}=9.56\times 10^{-2} M[/tex]
The reaction quotient is given as:
[tex]Q=\frac{[NOBr]^2}{[NO]^2[Br_2]}=\frac{(9.56\times 10^{-2} M)^2}{(2.69\times 10^{-2} M)^2\times 3.85\times 10^{-2} M}[/tex]
[tex]Q=328.06[/tex]
[tex]Q>K[/tex]
The reaction will go in backward direction in order to achieve an equilibrium state.
1. In order to reach equilibrium NOBr (g) must be produced. False
2. In order to reach equilibrium K must decrease. False
3. In order to reach equilibrium NO must be produced. True
4. Q. is less than K . False
5. The reaction is at equilibrium. No further reaction will occur. False
