Methyl iodide reacts irreversibly with azide ion with rate = k[CH3I][N3–]. CH3I(aq) + N3–(aq) → CH3N — Kinetics Chemistry Question
Question
Methyl iodide reacts irreversibly with azide ion with rate = k[CH3I][N3–].
CH3I(aq) + N3–(aq) → CH3N3(aq) + I–(aq)
The reaction is carried out with an initial concentration of CH3I of 0.01 M. Which statement about the reaction is correct?
A.
The time it takes for [CH3I] to decrease to 0.005 M is independent of [N3–], as long as [N3–] >> [CH3I].
B.✓ Correct
If the initial concentrations of azide and CH3I are equal, then it takes half as long for [CH3I] to decrease to 0.005 M as it does for it to decrease from 0.005 M to 0.0025 M.
C.
The reaction rate is significantly smaller if excess I– is added to the solution.
D.
The reaction cannot take place in a single elementary step.
💬
Still have doubts about this question?
Practice more questions like this, completely free.