what would be the rate of production for: (C6H5)CH2Cl ?
(C6H5)CH2SH ->k1 <-k-1 (C6H5)CH2+ + HS−
(C6H5)CH2+ + Cl− ->k2 (C6H5)CH2C
To determine the rate of production for (C6H5)CH2Cl, we need to understand the reaction mechanism described by the equations given. These equations represent a reaction between (C6H5)CH2SH and Cl−, which leads to the formation of (C6H5)CH2C.
The overall reaction can be represented as follows:
(C6H5)CH2SH + Cl− → (C6H5)CH2Cl + HS− (overall reaction)
The rate of production for (C6H5)CH2Cl is represented by the rate constant, k2. The rate of this reaction can be determined experimentally by measuring the change in concentration of (C6H5)CH2Cl over time. However, to calculate the rate constant, it would require additional information such as the concentration of reactants, temperature, etc., which may not be provided in the given information.
To experimentally determine the rate constant, you can perform multiple experiments, varying the concentrations of reactants, and measuring the change in concentration of (C6H5)CH2Cl over time. By plotting the concentration data and using a suitable rate equation, such as the rate equation derived from the rate-determining step of the reaction mechanism, you can obtain the rate constant (k2).
It's important to note that the rate constants k1 and k-1 represent the forward and reverse rate constants for the reaction between (C6H5)CH2SH and HS−, which are not directly related to the rate of production of (C6H5)CH2Cl.