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Theratelaw for thereaction C_(2)H_(4)Br_(2)+ 3I^(-) to C_(2) H_(4) + 2Br^(-)+ I_(3)^(-) isRate = k[C_(2)H_(4) Br_(2)][I^(-) ]. Therate of the reactionis found to be1.1 xx 10^(-4) M//s whenthe concentrations of C_(2) H_(4) Br_(2)and I^(-) are0.12 Mand 0.18 M respectively. Calculatethe rateconstantof thereaction. |
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Answer» Byrate LAW,Rateof REACTION `=R = k XX [ C_(2) H_(4) Br_(2) ][I^(-)]` `R= 1.1xx 10^(-4)Ms^(-1)` `[C_(2) H_(4)Br_(2) ]=0.12 M , [I^(-) ]= 0.18 M` Rateconstant = k = ? `R= k xx [C_(2)H_(4) Br_(2) ] xx [I^(-)]` `Ms^(-1)` `:. k= (R)/([C_(2) H_(4) Br_(2) ] xx [I^(-)])= (1.1 xx 10^(-4))/(underset(M)(0.12)xx underset(M)0.18) = 5.1 xx 10^(-3) M^(-1) s^(-1)` |
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