Question

Mechanism of the reaction $2NO+C{l}_2\to 2NOCl$ may be written as
$2NO\stackrel{K}{\rightleftharpoons }(NO{)}_2..........(fast)$

$(NO{)}_2+C{l}_2\stackrel{k}{⟶}2NOCl.......(slow)$
Rate equation would be:

• A. $kK\left[\right(NO{)}_2]\left[C{l}_2\right]$
• B. $kK{\left[NO\right]}^2\left[C{l}_2\right]$
• C. $kK\left[C{l}_2\right]$
• D. $kK\left[NO\right]\left[C{l}_2\right]$

Answer 1

The correct option is B $kK{\left[NO\right]}^2\left[C{l}_2\right]$

$r=k{\left[NO\right]}_2\left[C{l}_2\right]$
$K=\frac{{\left[NO\right]}_2}{{\left[NO\right]}^2}$
$r=kK{\left[NO\right]}^2\left[C{l}_2\right]$