1.

The reaction NO_(2(g))+O_((g)) to CO_(2(g)) +NO_((g)) proceeds in the following two steps at 500 K NO_(2(g)) + NO_2to NO+NO_3 Step - 1(slow) NO_3 + CO to CO_2 + NO_2 Step -2 (fast) Which of the following rate expressions is correct for the above reaction ?

Answer»

Rate `=-(d(NO_2])/(dt)=K[NO_2]`
Rate `=-(d[CO])/(dt) = k[NO_2]`
Rate `= -(d[NO_2])/(dt) =k[NO_2]^2`
Rate `=-(d[NO_2])/(dt) = k[NO_2][CO]`

SOLUTION :The rate expression in ACCORDING to the slow step of the reaction .
Rate = `(dx)/(dt) = k [NO_(2)]^(2)`


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