Determine the rate law and the value of k for the following reaction using the data provided: 2n2o5(g) → 4 no2(g) + o2(g)0.2241.16 x 10-3 a. rate = 5.6 × 10-2 m-1s-1[n2o5]2 b. rate = 6.0 × 10-1 m-2s-1[n2o5]3 c. rate = 1.6 × 10-3 m1/2s-1[n2o5]1/2 d. rate = 1.7 × 10-2 m-1/2s-1[n2o5]3/2 e. rate = 5.2 × 10⁻3 s-1[n2o5]

The rate law and the value of k is Rate = 5.2 x 10^-3 s-1[N2O5]

The rate law or rate equation for a chemical reaction is an equation that links the reaction rate with concentrations or pressures of reactants and constant parameters (normally rate coefficients and partial reaction orders).

The correct answer between all the choices given is the last choice or letter E. I am hoping that this answer has satisfied your query and it will be able to help you in your endeavor, and if you would like, feel free to ask another question.

can you list the answers so i can answer

since electrons are negative the answer is neagtaive