consider the following reactions and their respectiveequilibrium constants NO(g)

Question

consider the following reactions and their respectiveequilibrium constants NO(g)+ 1/2 Br2(g)<---> NOBr(g) 2NO(g)<--->N2(g)+ O2(g) calculate the value of the equilibrium constant for thereaction: N2(g)+O2(g)+Br2(g)<---> 2NOBr(g) K1= 5.3 K2= 2.1x1030 consider the following reactions and their respectiveequilibrium constants NO(g)+ 1/2 Br2(g)<---> NOBr(g) 2NO(g)<--->N2(g)+ O2(g) calculate the value of the equilibrium constant for thereaction: N2(g)+O2(g)+Br2(g)<---> 2NOBr(g) K1= 5.3 K2= 2.1x1030

Explanation / Answer

                 NO(g)+1/2 Br2(g)<---> NOBr(g)               K1 = [NOBr] / [NO][Br2]1/2                 2NO(g)<--->N2(g)+O2(g)                    K2 = [N2] [O2] /[NO]2         N2(g)+O2(g)+Br2(g)<---> 2NOBr(g)            K = [NOBr]2 / [N2] [O2] [Br2]                 = (K1)2 * 1 / K2                 = (5.3)2 * 1/2.1*1030                 =  13.37 * 10-30                         N2(g)+O2(g)+Br2(g)<---> 2NOBr(g)            K = [NOBr]2 / [N2] [O2] [Br2]                 = (K1)2 * 1 / K2                 = (5.3)2 * 1/2.1*1030                 =  13.37 * 10-30                                 = (5.3)2 * 1/2.1*1030                 =  13.37 * 10-30                                

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