Consider the following reaction: A+B→C+DA+B→C+D The initial concentrations of the reactants AA and BB are 0.260 M� and 0.400 M�, respectively. The rate of reaction is 0.060 M⋅s−1�⋅s−1, and the orders of the reaction, with respect to reactants AA and BB, are 1 and 2, respectively. Determine the rate constant (k�) for the reaction using the rate law.

KINETICS AND EQUILIBRIUM Identifying intermediates in a reaction mechanism Consider the following mechanism for the reduction of nitric oxide: H₂(g) + 2NO(g) → N₂O(g) + H₂O(g) H₂(g) + N₂O(g) → N₂(g) + H₂O(g) Write the chemical equation of the overall reaction: Are there any intermediates in this mechanism? If there are intermediates, write down their chemical formulas. Put a comma between each chemical formula, if there's more than one. ☐ yes no (1) (2) ローロ 00 09 0.0.... X Ś 0/3

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For the reaction: 3 Ag  +  NO3–  +  4 H+  –––>  NO  +  2 H2O  +  3 Ag+ If the rate of disappearance of Ag is 0.0017 mol L–1 s–1, what is the rate of the appearance of water? For the 1st order reaction:   A ––> products,    assume the concentration of A falls to one-third of its original value after 150 seconds.  Calculate the rate constant and the half-life.

Consider the following general reaction for which gases A and B are mixed in a constant volume container: A(g) + B(g) -> C(g) + D(g) Match what happens to the rate of the reaction under the following changes: (consider each change separately) v all of gas B is removed from the container more gas A is added to the container the temperature of the container is increased there is no change to the reaction rate ya catalyst is added to the container I. the reaction proceeds at a faster rate v gas D is also added to the container the reaction proceeds at a slower rate II. some of gas B is removed from the container Iy the reaction does not proceed at all the volume of the container is increased

17. SHOW ALL YOUR WORK OGiven the following data, determine the order of the reaction with respect to NO(g). 2 NO(g) + Cl2(g)→ 2 NOCI(g) Experiment 1 [C2] (M) 0.0100 [NO] (M) Rate (M/s) 3.4 x 104 1.36 x 103 3.4 x 104 0.0300 0.0150 0.0150 0.0100 3 0.0400

Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0092 M-s : 2 HI (g) - H, (g) +L, (g) Suppose a 450. mL flask is charged under these conditions with 150. mmol of hydrogen iodide. After how much time is there only 75.0 mmol left? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits. dlo x10 8. 미

6. The following data were obtained for the reaction: A → products. Determine the rate law for this reaction, including the value of k. [A] (M) time (s) 0.800 0 0.775 40 0.750 83 0.725 129 0.700 179

Consider the following reaction: A + B + C → D The rate law for this reaction is as follows: [A][C]* Rate = k [B]L/2 Suppose the rate of the reaction at certain initial concentrations of A, B, and C is 1.17x10-2 mol · L-ls¬1. Part A What is the rate of the reaction if the concentrations of A and C are doubled and the concentration of B is tripled? Templates Symbols uado redo reset keyboard shortcuts help Rate = mol · L-!s-1

Under certain conditions the rate of this reaction is zero order in dinitrogen monoxide with a rate constant of 0.0086 M's : 2 N,0 (g) → 2 N2 (g) + 0, (g) Suppose a 300. mL flask is charged under these conditions with 100. mmol of dinitrogen monoxide. How much is left 10. s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits. x10 미