The iodide ion reacts with hypochlorite ion (the active ingredient in chlorine bleaches) in the following way: OCl - + I - ¡OI - + Cl - . This rapid reaction gives the following rate data:
[OCl₄^-] (M) [I^-] (M) Initial Rate (M,s)
1.5 * 10-3 1.5 * 10-3
1.36 * 10-4 3.0 * 10-3 1.5 * 10-3 2.72 * 10-4
1.5 * 10-3 3.0 * 10-3 2.72 * 10-4
(b) Calculate the rate constant with proper units.

Question

The iodide ion reacts with hypochlorite ion (the active ingredient in chlorine bleaches) in the following way: OCl - + I - ¡OI - + Cl - . This rapid reaction gives the following rate data:

[OCl₄^-] (M) [I^-] (M) Initial Rate (M,s)

1.5 * 10-3 1.5 * 10-3

1.36 * 10-4 3.0 * 10-3 1.5 * 10-3 2.72 * 10-4

1.5 * 10-3 3.0 * 10-3 2.72 * 10-4

(b) Calculate the rate constant with proper units.

Accepted Answer

Hello, everyone. Today we have the following problem. The reaction of A C with B is as follows, given the following data showing the rate of the reaction. What is the rate constant of the reaction in proper units? So we have our rate law that can be written out, we have a rate law that can be written out as our rate is equal to some constant K times the concentration of A C which we can let X represent our A C and our B be represented by the exponent Y. And so we have to, let's first calculate the order with respect to A C. So with respect to A C, we have to look for data where the concentration of A sea changes while the concentration of the remains the same. And then we have to use their initial rates. So that's going to be, but where a sea changes is going to be from the first reaction to either the second or third. And then B is going to remain the same from the 1st and 3rd. So we're going to choose our top two there. So what we're gonna do is we're gonna have our reaction rates as 0.00094. Divided by 0.00047, equal to our concentration of A C For the first reaction, which is 0.008 divided by 0.004. And so we're gonna give those exponents as an ex there. When we plug into our calculator, this is actually going to be too, Is equal to two race of the power of X. And so what number can we put for X to give us two for both sides, X is going to equal one. So this is going to represent first order, this is our first order. And so now we have to calculate the order with respect to be, we're gonna do the same process. We're gonna look for the data where the concentration of B changes while the concentration of A remains the same. And that's going to be The 2nd and 3rd column here. And so we're gonna use the reaction rates once again, which was 0.94, divided by 0.47. And we're gonna divide that by the 0.008 and 0.004. And then once again, we're gonna use, why? Since this is B if we plug it into our calculator, we're going to get to is equal to two raised to the power of Y. Once again, Y is going to equal one. And this is going to be first order. So that's going to be first order plugging that into our rate law. We have some constant K times our A C race of the power of one times B raised to the power of one once again, which is essentially just going to be K times the concentration of A C times our concentration of B. And so we were just gonna use the first row to calculate for K. So we're gonna say that K is equal to our rate divided by our concentrations of A C times B. We set our rate For our first row is 0.00094 Mueller per second. And then our concentration of a was 0.0080. And then our concentration of B was 0.0040. And this is gonna give us a constant of 29.375. Moeller raised to the power of negative one times second race to the power of negative one as our final answer. And with that, we have answered the question overall, I hope this helped. And until next time.

Verified Solution

Key Concepts

Rate of Reaction

Rate Law

Units of the Rate Constant