‹ Back to the paper
Answer the following.
Consider the mechanism given below derived from spectrochemical analysis of the reaction between NO…
Consider the mechanism given below derived from spectrochemical analysis of the reaction between NO and $\mathrm{F_2}$:
$\mathrm{NO + F_2 \longrightarrow NOF_2}$ (slow step)
$\mathrm{NOF_2 + NO \longrightarrow 2NOF}$ (fast step)
The overall reaction is:
$\mathrm{2NO + F_2 \longrightarrow 2NOF}$
Calculate the number of times the rate of reaction will increase if the concentration of $[\mathrm{NO}]$ is doubled and the concentration of $[\mathrm{F_2}]$ is tripled.
Answer
Answer
AIRate $= k[\mathrm{NO}][\mathrm{F_2}]$
New rate $= k(2[\mathrm{NO}])(3[\mathrm{F_2}]) = 6k[\mathrm{NO}][\mathrm{F_2}]$
Final answer: 6
From ISC 2026 Improvement Chemistry Paper 1, question 2(iii).
Check your working with the Chemistry numericals calculator: solutions, electrochemistry and kinetics formulas: fill in what you know and get the rest.