From the table below, calculate : 1. The order of A 11. The order of B 111. The Rate Law 1. The Rate Constant v. Initial rate of experiment 4 Experiment number Initial [A]M - 1 0.033 Initial [B]M Initial Rate M/S 0.034 -4 6.67×10 -2 2 3 0.034 0.137 1.08×10 -2 0.136 0.136 1.07×10 4 0.202 0.233 ?

. For the following generic reaction: a A + b B -- > c C + d DWhat is the rate of reaction (rate expression) as a function of change in concentration (e.g. Δ[A]) andchange in time (Δt)?Describing Chemical Kinetics:1. Measuring RateThe rate of a chemical reaction is determined by:A. Change of moles of reactants/products over change in timeB. Change of grams of reactants/products over change in timeC. Change in concentration over change in timeD. change in volume over change in timeWrite the rate expressions based on the definition above for:a A + b B -- > c C + d Da A -- > productsDoes the order in reactant (m, n) in the rate law have anything to do with the coefficients of the reactants?

For a reaction in which A and B react to form C, the following initial rate data were obtained: Initial Rate of [A] [B] Formation of C (mol/L) (mol/L) (mol/L's) 0.10 0.10 1.00 0.10 0.20 4.00 0.20 0.20 8.00 What is the rate law? A. Rate=k[A]°[B] B. Rate=k[A][B]? C. Rate=k[A]°[B]? D. Rate=k[A]3 E. Rate=k[A][B] Reset Selection

The data for the reaction given NOCI (g) The following experimental data was measured for the reaction. Use the Method of Initial Rates to determine the rate law equation for this reaction 1 2 3 NO (g) + 1/2 Cl2₂ (g) [NO] [Cl₂] Initial Rate Experiment (mol.L-¹) (mol.L-¹) (mol.L-¹ s¯¹) 1.4x10-6 2.8x10-6 5.6x10-6 0.250 0.250 0.500 0.250 0.500 0.250 → 1. Determine the order of the reaction with respect to NO oxide 2. Determine the order of the reaction with respect to Cl₂ 3. What is the overall order of this reaction? 5. Calculate the value of the rate constant, k → 4. Select the correct rate law (rate equation) for this reaction: Rate =

43-46 Consider the time and concentration data for: 2 NO2(g) 2 NO(g) + O2(g). Time, s [NO2] 43 a. How long is the first half-life? Write the value and units 0.100 0.072 20 b. How long is the second half-life? Write the value and units 0.050 50 44. Write the rate law for this reaction. Explain why you made this choice. 0.036 90 0.025 150 45. What is the value of the rate constant? Write the general equation, the calculation equation with units, and the answer with units 46. How much time is needed until only 0.010 M NO2 remains? Write the general equation, the calculation with units, and the answer with units c

I need 21,22,23,24,25,26 answers