Question

The reaction $ A+2B+C\to Z $ occurs by the following mechanism : (i) $ A+B\xrightarrow{{}}''X'' $ (fast) (ii) $ X+C\xrightarrow{{}}Y $ (slow) (iii) $ V+B\xrightarrow{{}}X $ (very fast) Rate law for this reaction is:

• A. $ K[X][Y][Z] $
• B. $ K[Z] $
• C. $ K[A]{{[B]}^{2}}[C] $
• D. $ K[C] $

Answer 1

Answer: (D)

Slow step is the rate determining step of the reaction only in step (ii) the reaction 'C' is involved in the slow step.