Analyzing a new reaction Consider the following elementary steps that make up the mechanism of a certain reaction: 1. 2X→Y+Z 2. Y+ 2L¬M+Z Part A What is the overall reaction? Express your answer as a chemical equation. > View Available Hint(s)

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1) NO(g)  + O2 (g)  ><  NO3 (g)  2) NO3(g) + NO(g)  > <   2NO2(g0   for the reaction mechanism given, what is the rate law for each elementary equation? What is the rate law for the overall reaction if the mechanism is correct?

Nitrous oxide, NO, reacts with hydrogen to produce nitrogen and water. The initial rate data obtained for this reaction are given below: NO(g) + H2(g) –→ N2(g) + H2O(l) Using this data, determine the experimental rate law and calculate the rate constant. Experiment [NO] / mol L-1 [H2] / mol L-1 Initial Rate / mol L-1 s-1 1 0.420 0.122 0.136 0.210 0.122 0.0339 3 0.210 0.244 0.0678

1) Determine the order of the reaction and the rate constant. 2) What is the half-life of this reaction? 3) What is the concentration of the reactant after 2.00 hours of the experiment?

19. The initial rate of reaction between Substance A and Substance B was measured at a series of concentrations of each reactant with the following results. Solve for the rate law expression of this reaction. Note: Include all rough notes, show all calculations, follow the rules of significant figures, and box your final answer. ( A + B → AB Trial Number Trial #1 Trial #2 Trial #3 [A] 0.10 M 0.30 M 0.30 M [B] 0.10 M 0.10 M 0.20 M Initial rate 5.0 X 104 1.5 X 103 6.0 X 103 (mol/L·s)

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 =

A student wishes to experimentally determine the rate law of the following reaction. A+B+C+D The following tables demonstrate four students' plans for how to mix reactants and measure the rate of the reaction. Which can be used to determine the order of the reaction with respect to A and B? I. Trial 1 [A]initial 1M [B]initial 1M Trial 1 [A]initial 1 M [B]initial 3 M 2 1 M 1M III. 2 2 M 3 M 3 1 M 1 M 3 2 M 2 M Trial II. 1 1 M 2 1 M 1M 3 4 M 1 M [A]initial 2 M [B]initial IV. Trial [A]initial 1 1M [B]initial 1 M 2 1 M 1 M 3 2 M 2 M Table I only Table II only Table I & IV Table III only ○ Table II & III I don't know

Mechanism Suppose a reaction occurs with the following mechanism. All are elementary steps. Step 1: 0₂(9) 20(g) fast K₂ Step 2: O(g) + N₂(g) Step 3: O(g) + N(g) گی 3 NO(g) + N(g) slow very fast K3, NO(g) $ 4 % 5 6 What is the rate law for the rate-determining step? Rate =k,[0₂]² Rate = kr[O]² Rate-k,[O][N] Rate = kf[0₂]/k,[0]² Rate = k₂[O][N₂] Rate = K[0₂] & 7 What is the rate law for the forward reaction in step 1? Rate = kr[O]² Rate = kr[0₂] Rate =k+[0₂1² Rate = kr[0₂1² Rate = kf[0]² Rate =k+[0₂] What is the overall rate law for this reaction? Rate = k[N₂][0₂][N][0] MacBook Pro 8 ( 9 ☆ 88

The following initial rate data are for the reaction of ICI with hydrogen: 2IC1 + H₂ → I₂ + 2HCl Experiment [IC]o, M [H₂], M 0.198 0.141 0.396 0.141 0.198 0.281 0.396 0.281 1 2 3 4 Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = k = -2 M-². Initial Rate, M. s-¹ S 0.00657 0.0131 0.0261 0.0522 -1 S