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The data below were determined for the reaction shown below. S2O82– + 3I – (aq) → 2SO42– + I3–

[S2O82-] [I-] initial rate
1. 0.038 0.060 1.4x10^-5 M/s
2. 0.076 0.06 2.8x10^-5M/s
3. 0.076 0.03 1.4x10^-5 M/s
The rate law for this reaction must be:

1 Answer

4 votes

Answer:

k[S₂O₈⁻][I⁻].

Step-by-step explanation:

To solve this problem, I will rewrite the data for clarification:

Exp. [S₂O₈⁻],M [I⁻],M initial rate

1 0.038 0.060 1.4 x 10⁻⁵ M/s

2 0.076 0.060 2.8 x 10⁻⁵ M/s

3 0.076 0.030 1.4 x 10⁻⁵ M/s

The initial rate method to determine the order of the reaction is one of the most accurate methods to determine the order.

The rate law for this reaction = k[S₂O₈⁻]ᵃ[I⁻]ᵇ,

where, k is the rate constant of the reaction,

a is the order of the reaction with respect to [S₂O₈⁻].

b is the order of the reaction with respect to [I⁻].

From Exp 1 and 2,

The concentration of [S₂O₈⁻] changes while [I⁻] is constant, the initial rate of the reaction changes.

So, the rate of the reaction depends on [S₂O₈⁻].

(initial rate)₁ = k[S₂O₈⁻]₁ᵃ[I⁻]₁ᵇ (1)

(initial rate)₂ = k[S₂O₈⁻]₂ᵃ[I⁻]₂ᵇ (2)

By dividing (1) over (2)

∴ (initial rate)₁ / (initial rate)₂ = [k[S₂O₈⁻]₁ᵃ[I⁻]₁ᵇ] / [k[S₂O₈⁻]₂ᵃ[I⁻]₂ᵇ]

∴ (1.4 x 10⁻⁵ M/s) / (2.8 x 10⁻⁵ M/s) = [k[0.038]ᵃ[0.06]ᵇ] / [k[0.076]ᵃ[0.06]ᵇ]

∴ (0.5) = [0.038]ᵃ / [0.076]ᵃ = [0.5]ᵃ

Taking log for the both sides,

log (0.5) = a log (0.5)

∴ a = 1.

∴ the reaction is first order reaction with respect to [S₂O₈⁻].

From Exp. 2 and 3,

The concentration of [S₂O₈⁻] is constant while [I⁻] changes, the initial rate of the reaction changes.

So, the rate of the reaction depends on [I⁻].

(initial rate)₂ = k[S₂O₈⁻]₂ᵃ[I⁻]₂ᵇ (3)

(initial rate)₃ = k[S₂O₈⁻]₃ᵃ[I⁻]₃ᵇ (4)

By dividing (3) over (4)

∴ (initial rate)₂ / (initial rate)₃ = [k[S₂O₈⁻]₂ᵃ[I⁻]₂ᵇ] / [k[S₂O₈⁻]₃ᵃ[I⁻]₃ᵇ]

∴ (2.8 x 10⁻⁵ M/s) / (1.4 x 10⁻⁵ M/s) = [k[0.076]ᵃ[0.06]ᵇ] / [k[0.076]ᵃ[0.03]ᵇ]

∴ (2.0) = [0.06]ᵇ / [0.03]ᵇ = [2.0]ᵇ

Taking log for the both sides,

log (2.0) = a log (2.0)

∴ b = 1.

∴ the reaction is first order reaction with respect to [I⁻].

∴ the rate law for this reaction must be = k[S₂O₈⁻][I⁻].

User Codingwithmanny
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