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.

vanderwaal's forces of attraction are the electrostatic intermolecular forces that exist in a molecule due to the temporary or permanent dipoles that are developed in a molecule. in , the major intermolecular forces are dipole-dipole interactions as the molecule is polar (bent structure). so the vanderwaal's forces of interaction in between molecules are the permanent dipole-dipole interactions that develop due to the dipole that exists in between the polar h - s bond. the positively charged hydrogen atom is attracted towards the negative end of the dipole that is sulfur of the adjacent molecule. therefore, these forces of attraction are relatively stronger than that of london dispersion forces that exist in non polar molecules.