For the reaction C2H4Br2+ 3KI>C2H4+2KBr+KI3, when the rate of reaction is 2.0x10^-5, what is the rate of disappearance of KI?

To determine the rate of disappearance of KI, we need to look at the stoichiometry of the reaction. From the balanced equation:

C2H4Br2 + 3KI → C2H4 + 2KBr + KI3

We can see that for every 3 moles of KI, 1 mole of KI3 is produced. Therefore, the stoichiometric coefficient of KI is 3, meaning that for every mole of KI consumed, 3 moles of KI3 are formed.

The rate of disappearance of KI can be calculated by dividing the rate of reaction by the stoichiometric coefficient of KI. In this case, the rate of reaction is given as 2.0x10^-5. Therefore:

Rate of disappearance of KI = Rate of reaction / Stoichiometric coefficient of KI
= 2.0x10^-5 / 3
= 6.67x10^-6

Therefore, the rate of disappearance of KI is 6.67x10^-6.

To determine the rate of disappearance of KI, we need to examine the stoichiometry of the reaction. The balanced equation is:

C2H4Br2 + 3KI -> C2H4 + 2KBr + KI3

From the equation, we can see that the stoichiometric coefficient of KI is 3. This means that for every 3 moles of KI that react, 1 mole of KI3 is produced.

The question mentions that the rate of reaction is 2.0x10^-5, but it doesn't provide any additional information, such as the units of the rate. Therefore, we don't have enough information to directly calculate the rate of disappearance of KI.

However, if we assume that the given rate of reaction refers to the disappearance of either C2H4Br2 or KI (since they have stoichiometric coefficients of 1), we can use the stoichiometry of the reaction to calculate the rate of disappearance of KI.

Let's assume that the rate given refers to the disappearance of C2H4Br2. Since the stoichiometric coefficient of C2H4Br2 is 1, the rate of disappearance of KI can be calculated using the stoichiometric ratio:

rate_of_disappearance_KI = (1 mol KI3 / 3 mol KI) * rate_of_disappearance_C2H4Br2

If the given rate of reaction is indeed the rate of disappearance of C2H4Br2, we can substitute it into the equation to find the rate of disappearance of KI.

wouldn't it be three times the rate?

rate= -1/3 * d(KI)/dt

reat disappearance of KI=3*rate

(negative sign in the rate equation means reducing)

https://en.wikipedia.org/wiki/Reaction_rate