Question

determine the initial rate for a reaction that starts with 0.85 M of reagent A and 0.70 M of reagents B and C? Express your answer to two significant figures and include the appropriate units. Indicate the multiplication of units explicitly either with a multiplication dot or a dash.

For the reaction A+B+C→D+E, the initial reaction rate was measured for various initial concentrations of reactants. The following data were collected:

Trial [A](M) [B](M) [C](M) Initial rate (M/s)

1 0.30 0.30 0.30 9.0×10−5

2 0.30 0.30 0.90 2.7×10−4

3 0.60 0.30 0.30 3.6×10−4

4 0.60 0.60 0.30 3.6×10−4

(Reaction A is 2 order, Reaction B is 0 order, Reaction C is 1 order and k= 3.3*10^-3 M^-2s^-1 )

Answer 1

The reaction A+B+C→D+E

Given that; A is 2 order, Reaction B is 0 order, Reaction C is 1 order

Because when the concentration of A is doubles than the rate increase by4 fold.

when the concentration of B is doubles than there is no effect on the rate

when the concentration of C is doubles than the rate increase by 2 fold.

First calculate the value of rate constant ;k as follows:

Rate = k[A]^2[B]^0[C]^1

9.0*10^-5 M/s = k(0.30 M)^2 *(0.30M)^0*(0.30 M)^1

k = 9.0*10^-5 M/s / 0.027 M^-3

k = 3.33*10^-3 M^-2s^-1