He following mechanism has been proposed for the gas-phase reaction of chloroform (CHCl3) and chlorine. Cl2 ⇌ 2Cl (fast, reversible) Cl + CHCl3 → HCl + CCl3 (slow) Cl + CCl3 → CCl4 (fast) What rate law does this mechanism predict? (Choose from the list below and enter your answers in alphabetical order, e. g. ABC ). A)k G) [CCl3]1/2 M) [HCl]2 B) [Cl] H) [HCl]1/2 N) [Cl2]2 C) [CHCl3] I) [Cl2]1/2 O) [Cl]2 D) [CCl3] J) [Cl]1/2 P) [CHCl3]2 E) [HCl] K) [CHCl3]1/2 F) [Cl2] L) [CCl3]2 Tries 0/99 Decide which of the following reactive intermediates could exist for the reaction above. Cl Cl2 CHCl3 CCl3 CCl4 Tries 0/99

The rate law predicted by the given mechanism is ACI

Explanation:

In a mechanism of the reaction, the slow step in the mechanism determines the rate of the reaction.

The intermediate reaction of the mechanism follows:

Step 1:  

Step 2:  

Step 3:  

Overall reaction:  

As, step 2 is the slow step. It is the rate determining step

Rate law for the reaction follows:

     ......(1)

As, [Cl] is not appearing as a reactant in the overall reaction. So, we apply steady state approximation in it.

Applying steady state approximation for [Cl] from step 1 and step 3, we get:

Putting the value of [Cl] in equation 1, we get:

Hence, the rate law predicted by the given mechanism is ACI

c. because step up transformer steps up the input voltage i.e increases the input voltage  

the number of turns are greater on the secondary side of step up transformer  

transformer does not handle dc current

the number of valence electrons for each molecule or ion is shown beneath the structure. remember hydrogen will not have more than two electrons. this hydrogen is part of a covalent bond (sharing two electrons). a double bond here would cause hydrogen to share four electrons with phosphorus.