Question

H3AsO4 + 3I−+ 2 H3O+ H3AsO3 + I3− + H2O
The oxidation of iodide ions by arsenic acid in acidic aqueous solution occurs according to the stoichiometry shown above. The experimental rate law of the reaction is: Rate = k [H3AsO4] [I−] [H3O+]
25. What is the order of the reaction with respect to I−?
(A) 1 (B) 2 (C) 3 (D) 5 (E) 6

Answer 1

Answer:

• (A) 1

Explanation:

In a chemical reaction, the order of reaction with respect to one species is the exponent of the species in the rate law.

The experimental rate law of the reaction is:

        $rate=k[H_3AsO_4]\cdot [I^-]\cdot[H_3O^+]$

That means:

• k is the rate constant

• $[H_3AsO_4]$, $[I^-]$ , and $[H_3O^+]$ are the concentrations of the reactants

• The exponents are 1, 1, and 1.

• Thus, the order of the reaction with respect to each species is 1.

• The overall order is the sum of the exponents: 1 + 1 + 1 = 3.

In conclusion, the order of reaction with respect to  $[I^-]$ is 1.

Answer 2

The order of the reaction with respect to I− is 1.

The rate law shows the order of a given reaction in each of the reactants. For the reaction; H3AsO4 + 3I− + 2 H3O+ ------> H3AsO3 + I3− + H2O, we have the rate law; Rate = k [H3AsO4] [I−] [H3O+].

The interpretation of this is that the reaction is first order with respect to each of the reactants. Therefore, the order of the reaction with respect to I− is 1.

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