what would be the rate of production for: (C6H5)CH2Cl ?
(C6H5)CH2SH ->k1 <-k-1 (C6H5)CH2+ + HS−
(C6H5)CH2+ + Cl− ->k2 (C6H5)CH2C
please help how do i solve this question?
these are the options to choose from:
Rate= k1 k2 [ (C6H5)CH2SH ] [ Cl− ]k−1[ Cl− ]+k2[ HS− ]
Rate= k1 k2 [ (C6H5)CH2SH ] [ Cl− ]k−1[ HS− ]+k2[ Cl− ]
Rate=k1 k2k−1 [ (C6H5)CH2Cl ] [ HS− ][ (C6H5)CH2SH ] [ Cl− ]
Rate=k1k−1 [ (C6H5)CH2SH ] [ Cl− ]
Rate=(k1−k−1+k2) [ (C6H5)CH2SH ] [ Cl− ]
Rate=k1 k2k−1 [ (C6H5)CH2SH ] [Cl− ]
i have a similar problem and i got
Rate= k1 k2 [ (C6H5)CH2SH ] [ Cl− ]k−1[ HS− ]+k2[ Cl− ]
I think you have made a typo (at least one). Where did the intermeddiate HS^- go? Also I expect that in the second step that is supposed to be
(C6H5)CH2CH2Cl as the final product.
To solve this question, we need to use the rate law based on the given chemical equation. The rate law represents the relationship between the rate of a reaction and the concentrations of the reactants.
Let's analyze the given reaction:
(C6H5)CH2SH ->k1 <-k-1 (C6H5)CH2+ + HS−
(C6H5)CH2+ + Cl− ->k2 (C6H5)CH2Cl
The rate-determining step in this reaction is the second step, which involves the reaction between (C6H5)CH2+ and Cl− to form (C6H5)CH2Cl.
From the second step, we can identify the rate law expression:
Rate = k2 [ (C6H5)CH2+ ] [ Cl− ]
Now, we need to express [ (C6H5)CH2+ ] in terms of the other species present in the reaction. Referring back to the first step:
(C6H5)CH2SH ->k1 <-k-1 (C6H5)CH2+ + HS−
To calculate the concentration of (C6H5)CH2+, we need to know the concentration of (C6H5)CH2SH, which is not provided. So, we cannot directly determine the rate of production for (C6H5)CH2Cl from the given information.