Use the information below to determine the overall reaction order for A+B → C+D. Trial 1: [A] = 2.0 M, [B] = 1.0 M, rate = 0.10 M/s Trial 2: [A] = 6.0 M, [B] = 1.0 M, rate = • Trial 3: [A] = 2.0 M, [B] = 2.0 M, rate = ● Select the correct answer below: 2 3 = 0.10 M/s 0.40 M/s

Using the data in the table, calculate the rate constant of this reaction. k= = A + B → C + D Trial 1 2 3 Units [A] (M) [B] (M) 0.340 0.400 0.340 0.920 0.408 0.400 Rate (M/s) 0.0114 0.0603 0.0137

The data in the table below were obtained for the reaction: A + B → PRODUCT Experiment Number [A] (M) |[B] (M)| (M/s) |Initial Rate 1 0.273 0.763 2.83 0.273 1.526 2.83 0.819 0.763 25.47 The rate law for this reaction is rate =

A chemical reaction is characterized by the following experimental data: SO₂Cl2 → SO2 + Cl₂ [SO₂Cl₂] Time (mol L-¹) (min) 0.1000 0 0.0876 1.00 x 10² 0.0768 2.00 x 10² 3.00 x 10² 4.00 x 10² 5.00 x 10² 0.0673 0.0590 0.0517 6.00 x 10² 7.00 x 10² 8.00 x 10² 9.00 x 10² 1.000 x 10³ 0.0234 1.100 x 10³ 0.0453 0.0397 0.0348 0.0305 0.0267 First, graphically determine the instantaneous rate of decomposition of [SO₂Cl₂] using the tangent to the curve. Use scientific notation, e.g.enter 2E3 for 2000. Enter your answer with one significant figure. The decomposition rate: (A) at 200 min: i (B) at 600 min: i M/min M/min

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. d. The mechanism of the reaction is suggested as two steps: NO₂+ F2 → NO₂F + F (fast) NO₂+ F→→ NO₂F (slow) Is your rate law consistent with this mechanism? Explain your answer, making any changes necessary to create consistency.

[A] vs Time In[A] vs Time O 1/[A] vs Time Least Squares Plot The reaction A → C was performed and the concentration vs. time data below collected. time, s [A], mol/L 0.7983 0.1898 0.1077 0.07517 0.05774 0.04687 0.03944 0.03405 0.02995 [A] 0 reaction order = Check Submit Answer 1 Time, s 2 3 Try Another Version Complete the rate law for the reaction by filling in the values for the rate constant and reaction order. Rate = K[A]* rate constant (without units) = Next> (1 of 1) Show Approach 2 item att 5 6 Hide Hint 7 8 A least squares line gives the best straight- line fit through any set of points but to get the right answer you need to figure out which plot gives the straight line.

Consider the gas phase reaction 2 NO + H₂ → N₂O + H₂O The experimental rate law is found to be R = [NO]²[H₂] Which of the mechanisms shown below is consistent with the information about this reaction given in this question? Step 1: NO + H₂ → N + H₂O (slow) Step2: N + NO → N₂O (fast) Step 1: NO + NO 2 NO₂ + N (slow) (fast) Step2: NO₂ + H₂ Step 3: N + NO → NO + H₂O N₂O (fast) Step 1: NO + NO>>> N₂O₂ Step2: N₂O₂ + H2 →→ N₂O + H₂O 2H (fast) Step 1: H₂ Step2: H+2 NO → Step 3: H+ OH → N₂O + OH (slow) H₂O (fast) (fast) (slow)

Use the information below to determine the overall reaction order for A + B → C+D. Trial 1: [A] = 3.0 M, [B] = 3.0 M, rate = 0.10 M/S Trial 2: [A] 6.0 M, [B] = 3.0 M, rate = 0.40 M/S Trial 3: [A] = 3.0 M, [B] = 6.0 M, rate = 0.40 M/s Select the correct answer below: O 1 2 3 4