• # question_answer In the reversible reaction$2N{{O}_{2}}{{N}_{2}}{{O}_{4}}$ the rate of disappearance of $N{{O}_{2}}$ is equal to A)  $\frac{2{{k}_{1}}}{{{k}_{2}}}\,{{\left[ N{{O}_{2}} \right]}^{2}}$B)  $2{{k}_{1}}{{[N{{O}_{2}}]}^{2}}-2{{k}_{2}}[{{N}_{2}}{{O}_{4}}]$C)  $2{{k}_{1}}{{[N{{O}_{2}}]}^{2}}-{{k}_{2}}[{{N}_{2}}{{O}_{4}}]$D)  $(2{{k}_{1}}-{{k}_{2}})\,[N{{O}_{2}}]$

$2N{{O}_{2}}{{N}_{2}}{{O}_{4}}$ Rate $=\frac{1}{2}\frac{d\,[N{{O}_{2}}]}{dt}$ $={{k}_{1}}{{[N{{O}_{2}}]}^{2}}-{{k}_{2}}[{{N}_{2}}{{O}_{4}}]$ Rate of disappearance of $N{{O}_{2}}$ i.e.             $-\frac{d[N{{O}_{2}}]}{dt}=2{{k}_{1}}\,\,{{[N{{O}_{2}}]}^{2}}-2{{k}_{2}}[{{N}_{2}}{{O}_{4}}]$