For the reaction

2A(g)+2B(g)+C(g)⟶3G(g)+4F(g)

the initial rate data in the table was collected, where [A]0 , [B]0 , and [C]0 are the initial concentrations of A , B , and C , respectively.

Experiment [A]0 (mmol⋅L−1) [B]0 (mmol⋅L−1) [C]0 (mmol⋅L−1) Initial rate (mmol⋅L−1⋅s−1)
1 11.0. 200.0 220.0 8.80
2 22.0 200.0 165.0 17.6
3 22.0 400.0 55.0 70.4
4 11.0 200.0 110.0 8.80

Reactant A is first order reactant, Reactant B is second order reactant, and Reactant C is zero order reactant...

1. What is the overall order of the reaction ____ ???
2. Write the rate law for the reaction where is the rate constant. Rate = k_???
3. Calculate the rate constant, , and identify its units. K = ?????
4. Determine the initial rate of the reaction when [A]0=4.87 mmol⋅L−1 , [B]0=0.184 mmol⋅L−1 , and [C]0=12.0 mmol⋅L−1 . Initial Rate = ___ mmol⋅L−1⋅s−1 ??????

1) The order of reactant A is first order reactant because a first-order reaction can be defined as a chemical reaction in which the reaction rate is linearly dependent on the concentration of only one reactant.

The order of reactant B is second order reactant because a second order reaction is a type of chemical reaction that depends on the concentrations of one-second order reactant or two first-order reactants.

Thus, the overall order of the reaction is 3.

2) The rate law in this reaction is;

rate = [A]^n [B]^m [C]^l

But in this question, since the reactant C is zero order, then it will be simplified to; rate = k[A][B]² .

3) When we plug in the initial concentrations of A and B, we will get the rate constant of the problem which is k = 20.

4) The initial rate when [A]0=4.87 mmol⋅L−1 , [B]0=0.184 mmol⋅L−1 , and [C]0=12.0 mmol⋅L−1 is;

Rate = 20 * 4.87 * 0.184²

Rate = 3.3

Read more about Order of Reaction at; https://brainly.com/question/16416932

#SPJ1