What is the rate law of the following reaction assuming it follows an elementary rate equation.  CH4 + 2O2 --> CO2 + 2H2

Consider the data table below for the generic reaction A + B → products Trial [A] (M) [B] (M) Rate (M/s) 1 0.150 0.100 9.00×10−4 2 0.150 0.200 1.80×10−3 3 0.300 0.100 3.60×10−3 4 0.600 0.200 2.88×10−2 Determine the rate law for the reaction. (You do not need to calculate ) Show your work or explain your reasoning. What are the units of and how do you know?

A chemical engineer is studying the rate of this reaction. 2Cl,0, (g) → 2Cl, (g) + 50, (g) He fills a reaction vessel with Cl,O, and measures its concentration as the reaction proceeds. Here's a graph of his data: 0.2 0.15 0.1 0.05 0.02 0.04 0.06 0.08 0.1 (s)

step elementary reaction rate constant 1 NO₂(g) + F₂(g) → k₁ 2 F (g) + NO₂(g) NO₂F (g) k₂ Suppose also k₁k2. That is, the first step is much faster than the second. Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical reaction. rate = k Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of K₁, K2, and (if necessary) the rate constants k-1 and k-2 for the reverse of the two elementary reactions in the mechanism. k = 0 NO₂F(g) + F(g) 0-0 믐 010 X

For the reaction 2A(g) +3B(g) → C(g) + 3D(g) the following data was collected at constant temperature. Determine the correct rate law for this reaction. Trial Initial [A] Initial [B] Initial Rate (mol/L) (mol/L) (mol/(L·min)) 1 0.100 0.100 1.50 x 10-2 2 0.100 0.200 6.00 x 10-2 3 0.200 0.100 1.20 x 10-1 rate = k[A][B] rate = k[A][B]² rate= k[A]³[B]² rate= k[A] 1.5[B] rate = k[A][B]

A reaction mechanism has the following proposed elementary steps: Step 1: A ⇌ B + C Step 2: A + B → D Step 3: 2 A + D → C + E Which of the following equations would represent the overall reaction for this mechanism? Which species are intermediates in this reaction? Which of the following would be the correct elementary rate law for Step 1? Which of the following would be the correct elementary rate law for Step 2? Which of the following would be the correct elementary rate law for Step 3? If Step 1 is the rate-limiting step, what would the proposed rate law for this mechanism be? If Step 2 is the rate-limiting step, what would the proposed rate law for this mechanism be?

Given the following rate and concentration data, determine the rate law for the reaction A + B ---> products [A]0 (M) [B]0 (M) initial rate (M/s) 0.10 0.10 4.22 X 10^-6 0.20 0.10 8.44 X 10^-6 0.20 0.40 3.38 X 10^-6 the rate constant k= rate=

IReview | Constants | Periodic Table Order and rate law of a reaction The overall order of an elementary step directly corresponds to its molecularity. Both steps in this example are second order because they are each bimolecular. Furthermore, the rate law can be determined directly from the number of each type of molecule in an elementary step. For example, the rate law for step 1 is rate = k[NO2]? The exponent "2" is used because the reaction involves two NO2 molecules. The rate law for step 2 is rate = k[NO3]*[CO] = k[NO3][CO] because the reaction involves only one molecule of each reactant the exponents are omitted. Analyzing a new reaction Consider the following elementary steps that make up the mechanism of a certain reaction: 1. 3A B+ C 2. B+ 2D C+F Part A What is the overall reaction? Express your answer as a chemical equation. > View Available Hint(s) ΑΣφ ***** 2:55 PM 53°C Cloudy

NO2 + CO​NO + CO2 a -the rate law of this reaction

2 NO(g) + Br2 (g) → 2 NOB1(g) Initial Rate Experiment NO] (M) [Br2] (M) (mol/L's) 1 1.0 x 10-2 2.0 × 10-2 2.4 x 10-2 2 4.0 x 10-2 2.0 × 10-2 0.384 3 1.0 x 10-2 6.0 x 10-2 7.2 x 10-2 What is the order of the reaction with respect to [NO] and [Br2], and what is the overall order of the reaction? Order with respect to [NO] = Order with respect to [Br2] = Overall order