Question

Mechanism of the reaction $2NO + Cl_2 \to 2NOCl$ may be written as
$2NO \xrightleftharpoons{K}(NO)_2 .......(fast)$
$(NO)_2+CI_2 \rightleftharpoons{K}2NOCl .......(slow)$
Rate equation would be

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

Answer 1

Answer: (B)

$r=k\left[NO\right]_{2}\left[Cl_{2}\right]$
$K=\frac{\left[NO\right]_{2}}{\left[NO\right]^{2}}$
$r=kK\left[NO\right]^{2}\left[Cl_{2}\right]$