Question

For the reaction: c2h4br2 + 3 ki → c2h4 + 2 kbr + ki3, when the rate of disappearance of c2h4br2 is 2.0 × 10-5 m/s, what is the rate of disappearance of ki?

Answer 1

Answer: The value of the rate disappearace of KI is
`6.0* 10^(-5)`

Step-by-step explanation:

Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.

`C_2H_4Br_2+3KI\rightarrow C_2H_4+2KBr+KI_3`

The rate in terms of reactants is given as negative as the concentration of reactants is decreasing with time whereas the rate in terms of products is given as positive as the concentration of products is increasing with time.
`Rate=-(1d[C_2H_4Br_2])/(dt)=-(1d[KI])/(3dt)=`

Given:
`(d[C_2H_4Br_2])/(dt)]=2.0* 10^(-5)`

Putting in the values we get:

Rateof disappearace of KI=
`3* 2.0* 10^(-5)=6.0* 10^(-5)`

Thus the value of the rate disappearace of KI is
`6.0* 10^(-5)`