Consider the following reactions and their equilibriumconstants: NO (g) + 1/2 Br

Question

Consider the following reactions and their equilibriumconstants: NO(g) + 1/2 Br2 (g) <-->NOBr(g)    Kp= 5.3 2NO(g) <--> N2(g) +O2(g)     Kp= 2.1 x1030 Use these reactions and their equilibrium constants to predictthe equilibrium constant for the following reaction:       N2(g) +O2(g) + Br2(g) <-->2NOBr(g) Consider the following reactions and their equilibriumconstants: NO(g) + 1/2 Br2 (g) <-->NOBr(g)    Kp= 5.3 2NO(g) <--> N2(g) +O2(g)     Kp= 2.1 x1030 Use these reactions and their equilibrium constants to predictthe equilibrium constant for the following reaction:       N2(g) +O2(g) + Br2(g) <-->2NOBr(g) Use these reactions and their equilibrium constants to predictthe equilibrium constant for the following reaction:       N2(g) +O2(g) + Br2(g) <-->2NOBr(g)

Explanation / Answer

NO(g) + 1/2 Br2 (g) <-->NOBr(g)    Kp 1 = 5.3 Kp1 = p NOBr / ( p NO * p 1/2 Br2 ) ----(1) 2NO(g) <--> N2(g) +O2(g)     Kp 2 = 2.1 x1030 Kp 2 = ( p N2 * p O2 ) / p 2NO     ----(2 )    N2(g) + O2(g) +Br2(g) <--> 2NOBr(g) The Kp for the reaction is given by Kp = p 2 NOBr / ( p N2 * p O2 * p Br2 )                                                           = ( p NOBr / ( p NO * p 1/2 Br2 ) )2 * ( 1 / ( p N2 * p O2 ) / p 2NO     )                                                            =(  Kp 1 ) 2 * (1/  Kp 2 )                                                           = 5.3 2 / 2.1 * 10^ 30                                                           = 13.376 * 10^-30

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