The rate of a certain reaction is given by the following rate law: = K[N₂]³[0₁] Use this information to answer the questions below. rate = k What is the eaction order in N₂? What is the reaction order in 03? What is overall reaction order? At a certain concentration of N₂ and O3, the initial rate of reaction is 45.0 M/s. What would the initial rate of the reaction be if the concentration of N₂ were doubled? Round your answer to 3 significant digits. The rate of the reaction is measured to be 8.0 x 103 M/S when [N₂] = 1.5 M and [03] = 0.42 M. Calculate the value of the rate constant. Round your answer to 2 significant digits. 0 0 0 WO -3 k= <= M²³ · S -1 S 0

8. For a certain reaction, the reaction rate in terms of the change in concentration with time for each substance is: 1 A[O,] 5 At 1 A[NH3] 1 A[NO]_ 1 A[H,O] Rate 4 At 4 At 6 At A. Write a balanced equation for this gaseous reaction. B. When [H2O] is increasing at a rate of 2.523 mol/L-s, how fast is [O2] decreasing?

= O KINETICS AND EQUILIBRIUM Using a rate law The rate of a certain reaction is given by the following rate law: rate = k [NO] ² [0₂] Use this information to answer the questions below. What is the reaction order in NO? What is the reaction order in O₂? What is overall reaction order? At a certain concentration of NO and O₂, the initial rate of reaction is 0.750 M/s. What would the initial rate of the reaction be if the concentration of NO were doubled? Be sure your answer has the correct number of significant digits. The rate of the reaction is measured to be 99.0 M/s when [NO] = 0.62 M and [0₂] = 1.1 M. Calculate the value of the rate constant. Be sure your answer has the correct number of significant digits. 0 0 -2 -1 k = 0 M²³².5²² x10 X 5 0/5

Some measurements of the initial rate of a certain reaction are given in the table below. [₂] [H₂] initial rate of reaction 0.256M 1.41 M 6.00 × 10³ M/s 0.0501 M 1.41 M 230.M/s 0.256M 0.245 M 1.04 × 10³ M/s to write a rate law for this reaction, and calculate the value of Use this information the rate constant k. Round your value for the rate constant to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = kx k = 0 10⁰ ☐ x10 0.0 X

The rate of a certain reaction is given by the following rate law: rate =k[N_] [H,° Use this information to answer the questions below. What is the reaction order in N2? What is the reaction order in H2? What is overall reaction order? At a certain concentration of N2 and H2, the initial rate of reaction is 0.260 M/ s. What would the initial rate of the reaction be if the concentration of N2 were doubled? Be sure your answer has the correct number of significant digits. M The rate of the reaction is measured to be 8.0 x 103 M/s when [N2] = 0.58 M and [H2] = 2.0 M. Calculate the value of the rate constant. Be sure your answer has the correct number of significant digits. -3 -1 k = |M

A chemical reaction has the rate law R k[A]²[B] The rate of the reaction is found to be 4.3 M/min when the [A] = 0.20 M and [B] = 0.10 M. What is the value of the rate constant? k = 1.1 x 10³ M-¹ min-¹ none of the answers are correct = O k = 1.1 x 10³ M min-¹ O k = 1.1 x 10³ M-² min-¹

A reaction has a rate constant, k = 1.29 s-1. What is the half-life (seconds) when the initial concentration is 0.784 M?

The rate of a certain reaction is given by the following rate law: e=k [NO] ² [0₂] Use this information to answer the questions below. What is the reaction order in NO? What is the reaction order in O₂? What is overall reaction order? At a certain concentration of NO and O₂, the initial rate of reaction is 0.510 M/s. What would the initial rate of the reaction be if the concentration of NO were halved? Round your answer to 3 significant digits. The rate of the reaction is measured to be 29.0 M/s when [NO] = 0.55 M and [0₂] = 1.7 M. Calculate the value of the rate constant. Round your answer to 2 significant digits. 2 1 3 M S -2 -1 k = M ²² ₁5² ¹ □ x10 X Ś ?

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Some measurements of the initial rate of a certain reaction are given in the table below. [N₂] [H₂] initial rate of reaction 0.496M 1.63 M 6.00 × 10³ M/s 0.496M 0.191M 82.4M/s 0.209M 1.63 M 2.53 × 10³ M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = k k = | x10 ロ・ロ X