Answer :
Identification of comparison pairs for the determination of each exponent: First comparison pair for exponent a = A2 / A1 Second comparison pair for exponent a = A3 / A1 Third comparison pair for exponent a = A3 / A2 First comparison pair for exponent b = A4 / A1 Second comparison pair for exponent b = A5 / A1.
Third comparison pair for exponent b = A5 / A4 First comparison pair for exponent c = A6 / A1 Second comparison pair for exponent c = A7 / A1 Third comparison pair for exponent c = A7 / A6For the initial rate, the exponents are represented by a, b, and c. Using the above comparison pairs, we can identify the values of these exponents. So, we can see from the above pairs:
A2 / A1 = k [I-]a[BrO3-]b[H+]cA3 / A1 = k [I-]a[BrO3-]b[H+]c / k [I-]a[BrO3-]b[H+]c = A3 / A2 = k [I-]a[BrO3-]b[A7 / A1] / [A6 / A1] = k [I-]a[BrO3-]b[H+]c / k [I-]a[BrO3-]b[H+]c = A7 / A6.
From the above comparisons, the values of exponents a, b, and c are:
A2 / A1 = (I-)A3 / A2 = (BrO3-)^(-1)A3 / A1 = (I-)(BrO3-)^(-1)A4 / A1 = (BrO3-)A5 / A1 = (I-)(BrO3-)A5 / A4 = (I-)A6 / A1 = (S2O3(2-))^(-1)A7 / A1 = (H+)A7 / A6 = (S2O3(2-))^(-1)
So, the rate law for the iodine-clock reaction is:
Rate: k [I-]^1[BrO3-]^(-1)[S2O3(2-)]^(-1)[H+]^1
Also, the average value of the rate-constant determinations, with three significant figures, is 0.449. The rate law of the iodine-clock reaction is:
Rate = k [I-]^1[BrO3-]^(-1)[S2O3(2-)]^(-1)[H+]^1.
The value of the rate constant is 0.449. This question is related to the iodine-clock reaction in which iodine is produced. The reaction between potassium iodate, potassium iodide, and sulfuric acid in the presence of starch leads to the production of iodine. This reaction is referred to as the iodine-clock reaction since iodine is generated suddenly and gives a blue-black colour in the presence of starch.There are two steps involved in this reaction, with the first step being the reaction between potassium iodate and iodide ions. The iodide ions act as a catalyst for this reaction. Iodate ions are reduced to iodine in the second step by hydrogen peroxide produced in the first step. This reaction is a redox reaction since there is a transfer of electrons between species. The reaction's rate law and rate constant can be determined by measuring the reaction rate under different conditions and determining the reaction order of each species. The rate law for this reaction is given as:
Rate = k [I-]^1[BrO3-]^(-1)[S2O3(2-)]^(-1)[H+]^1
The reaction order of I- is 1, the reaction order of BrO3- is -1, the reaction order of S2O32- is -1, and the reaction order of H+ is 1. The value of the rate constant is 0.449. This iodine-clock reaction is a demonstration of the effect of concentration and temperature on the rate of a chemical reaction.
The conclusion is that the reaction order of I- is 1, the reaction order of BrO3- is -1, the reaction order of S2O32- is -1, and the reaction order of H+ is 1.
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