10. The data below are for the reaction: 2 NO₂ (g) + F₂ (g) → 2 NO₂F (g) [NO₂] (M) 0.100 0.200 0.200 0.400 0.200 [F₂] (M) 0.100 0.100 0.200 0.400 0.400 Initial rate (M/s) 0.026 0.051 0.103 0.411 see part c a. Write the rate law for this reaction. b. Determine the rate constant for this reaction. Pay attention to units. c. Predict the initial rate of the reaction when [NO₂] = 0.200 M and [F₂] = 0.400 M.

A chemistry graduate student is studying the rate of this reaction: 2SO3 (g) 2So, (g) +0, (g) He fills a reaction vessel with SO, and measures its concentration as the reaction proceeds: time [so,] olo (seconds) 18 0.200M Ar 0.10 0.127M 0.20 0.0805 M 0.30 0.0511 M 0.40 0.0324M Use this data to answer the following questions. Write the rate law for this reaction. rate = k|| x10 Calculate the value of the rate constant k.

Initialte data a centain empera - fat rafe tuse is given in He table forr the the fable for the followingreactim. Determine the pate constont, Ko नाप the value and emits of

Please show all steps

Consider the following reaction and information:   A + 2B → 3C rate = k{B}   Time (min.) B (M) A (M)0 0.72 0.5030 0.25 0.2660 0.087 0.18 What is the concentration of B after 27 minutes?

How do you determine the overall order of the reaction?

25. Nitrogen(II) oxide reacts with chlorine according to the equation: 2NO(g) + Cl₂(g) →→→ 2NOCI(g) The following initial rates of reaction have been observed for certain reactant concentrations: [NO] (mol/L¹) [Cl₂] (mol/L) Rate (mol/L/h) 0.50 1.00 1.00 0.50 0.50 1.00 1.14 O 4.56 9.12 What is the rate equation that describes the rate's dependence on the concentrations of NO and Cl₂? What is the rate constant? What are the orders with respect to each reactant? S N

Some measurements of the initial rate of a certain reaction are given in the table below. [H2] [12] initial rate of reaction 2.42M 1.68 M 0.0836M/s 2.42M 3.71 M 0.185 M/s 0.848 M 1.68 M 0.0293 M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = k☐ k = = 0 x10 ☐ □·□

Consider the hypothetical reaction 4A + 3B – 2C + D A certain amount of A and B was placed in a container and the reaction was allowed to proceed. The initial concentration of the products is zero. Over an interval of 1.5 s the average rate of change of the concentration of B was measured to be -0.0800 M/s. What is the concentration of D at the end of this same interval. 0.10 M 0.04 M 0.02 M 0.12M O O O

Calculate the average reaction rate for each time interval in moles of NO2 produced per liter per minute. 0-100 s 500-600 s 1100-1200 s