Can I get detailed explanation on 5 factors affecting rate of a reaction with diagrams if possible for my better understanding

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Part E The gas-phase reaction of N0 with F2 to form NOF and F has an activation energy of Ea = 6.30 Given that dashed lines indicate the weak bonds that are beginning to form, which is the most probable transition state for the formation of NOF? kJ/mol and a frequency factor of A = 6.00x108 M-1.s-1 . The reaction is believed to be •S • View Available Hint(s) bimolecular: NO(g) +F2(g)→NOF(g)+F(g) Ö=N. F-F :Ö=N: F-F :Ö=N: F-F F-F

Please explain how to find rate constant (k) if  reaction rate = 3.40*10^-7 I^- molar = .00200 (reaction order 1) BrO3^- molar = .00800 (reaction order 1) H^+ molar = .0400 (reaction order 2)

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Final Reactant Concentrations and Reaction Rates   [I-] [BrO3-] [H+] Reaction Time Rate of Reaction 2.8 x 10-5/time Expt. # M M M sec. M/sec 1 0.00166 0.0066 0.0166 258   2 0.0033 0.0666 0.0166 135   3 0.00166 0.0133 0.0166 132   4 0.00166 0.0066 0.033 78   FIND THE RATE?

Write a balanced reaction for which the following rate relationships are true. Rate (A[NO]/At) = - (1/2)(A[HNO3]/At) = (A[H₂O]/At) = (1/3)(A[NO₂]/At) No +해 + + HNO3 H₂O 1 NO₂ 6 NO3HNO3 6H 20 + 2NO₂ If the rate of disappearance of NO in the reaction in #1 is 0.270 M s-1 at 150°C, the rate of appearance of NO3 is. What is the overall order of the reaction in #1, if given is the rate law? Rate = k[NO]2 [HNO3]³ Ms-1 Given the above rate law, how does the rate of reaction change if the concentration HNO3 is doubled? ANSWER:

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