For the reaction, A+2B +C to D +2E, the rate of formation of D is found to be i)doubled when [A] is doubled keeping [B] and [C] constant ii)doubled when [C] is doubled keeping [A] and [B] constant iii) the same when [B] is doubled keeping [A] adn [C] constant. Which one is the rate equation for the reaction

For the reaction, A+2B +C to D +2E, the rate of formation of D is foun

1.	For the reaction, A+2B +C to D +2E, the rate of formation of D is found to be i)doubled when [A] is doubled keeping [B] and [C] constant ii)doubled when [C] is doubled keeping [A] and [B] constant iii) the same when [B] is doubled keeping [A] adn [C] constant. Which one is the rate equation for the reaction
Answer» rate `=k[A] [B] [C]` rate `=k [A]^0[B] [C]` rate `=k[A] [B]^0[C]` rate `=[A][B][C]^0` Solution :The given reaction is Ist order in A because on doubling the concentration of A because on doubling the concentration of A, rate of formation of 'D' is DOUBLED. Similary, if is FIRST order in C. But, the reaction is zero order in B because the doubling of its concentration does not affect the reaction rate. So, the rate eqaution for the reaction BECOMES, `(dx)/(DT)=k[A][B]^0[C]`