Question

Iodide ion (I−) reacts with hydrogen peroxide (H₂O₂ with a rate constant of 0.0133 M−1s−1 at 25°C. The values for x and y in the rate law equation are both egual to 1. What concentration of iodide ion should be added to 1.5 M H2O2 to achieve a rate of reaction equal to 6.0 × 10−4 M/s?

Answer 1

You need to add 2.83 × 10⁻² M of iodide ion to achieve the desired rate of reaction.

Step-by-step explanation:

This question is about determining the concentration of iodide ion needed to achieve a desired reaction rate in a reaction between iodide ion and hydrogen peroxide. It focuses on the application of the rate law equation and the concept of rate constant.

Solving for the concentration of iodide ion

1. Identify the rate law equation:

Given x = y = 1, the rate law equation becomes:

rate = k[I-][H2O2]

2. Plug in known values:

k = 0.0133 M⁻¹s⁻¹

[H2O2] = 1.5 M

Desired rate = 6.0 × 10⁻⁴ M/s

3. Set up the equation:

6.0 × 10⁻⁴ M/s = 0.0133 M⁻¹s⁻¹ * [I-] * 1.5 M

4. Solve for [I-]

[I-] = (6.0 × 10⁻⁴ M/s) / (0.0133 M⁻¹s⁻¹ * 1.5 M)

[I-] ≈ 2.83 × 10⁻² M

Therefore, you need to add 2.83 × 10⁻² M of iodide ion to achieve the desired rate of reaction.