Suppose the synthesis of ethylene dichloride proceeds by the following mechanism

Question

Suppose the synthesis of ethylene dichloride proceeds by the following mechanism: elementary reaction CH-CH2 (g) +Cl2 (g) CH-CH-Cl+(g) +Cl-(g)| CH-CH.Cl1@-cl-(g) CH-CH-Cl2 (g) Suppose also kl k2. That is, the first step is much slower than the second. step rate constant 1 | Write the balanced chemical equation for the overall chemical reaction Write the experimentally- observable rate law for the overall chemical reaction. = k Note: your answer should not contain the concentrations of any intermediates. contel your answer should not rate D

Explanation / Answer

1)
overall reaction is obtained by adding both steps
CH2CH2 (g) + Cl2 (g) —> CH2CH2Cl2 (g)
2)
here 1st step is lowest step
Rate depends on slowest step
so, rate law is:
rate = k [CH2CH2][Cl2]

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