Using a rate law The rate of a certain reaction is given by the following rate law: e=k[N₂] [H₂]² 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 0.700 M/s. What would the initial rate of the reaction be if the concentration of N₂ were halved? Round your answer to 3 significant digits. The rate of the reaction is measured to be 20.0 M/s when [N₂] = 0.27 M and [H₂] = 0.49 M. Calculate the value of the rate constant. Round your answer to 2 significant digits. 1 2 3 0 M -2 -1 k= M²²-5¹ 0 x10 X Ś

Use this information to write a rate law for this reaction, and calculate the value of the rate constant, k.

The rate of a certain reaction is given by the following rate law: = K[H₂] [¹₂] Use this information to answer the questions below. rate= What is the reaction order in H₂? What is the reaction order in 1₂? What is overall reaction order? At a certain concentration of H₂ and I2, the initial rate of reaction is 85.0 M/s. What would the initial rate of the reaction be if the concentration of H₂ were doubled? Round your answer to 3 significant digits. The rate of the reaction is measured to be 0.110 M/s when [H₂] = 1.3 M and [1₂] = 1.4 M. Calculate the value of the rate constant. Round your answer to 2 significant digits. k = Ом M 0 M 04/ S 'S -1 0x10 X

15.Study the reaction and read the statement. 2A + 3B + C →→  D + E  The rate constant for this reaction is 0.25. The reaction is second order in A and first order in B and C.  What is the rate of the reaction if [A] is 0.4 M, [B] is 0.1 M and [C] is 0.2 M? a.5.0 × 10–4   b.4.0 × 10–3   c.2.0 × 10–3   d.8.0 × 10–4

Some measurements of the initial rate of a certain reaction are given in the table below. [N₂] [H₂] initial rate of reaction 1.81M 0.376M 105 M/s 1.81M 0.0561 M 1.19 × 105 M/S 0.236M 0.376M 1.36 × 104 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 = k0.0² 0 8.00 × k = x10 0.0 X

The rate of a certain reaction is given by the following rate law: rate = k = K[N₂] ² [H₂1² 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 0.520 M/s. What would the initial rate of the reaction be if the concentration of N₂ were halved? Round your answer to 3 significant digits. The rate of the reaction is measured to be 5.0 x 10³ M/s when [N₂] = 1.3 M and [H₂] = 1.5 M. Calculate the value of the rate constant. Round your answer to 2 significant digits. k = M 'S M S X

The rate of a certain reaction is given by the following rate law: rate =k[H,T[NH3 Use this information to answer the questions below. What is the reaction order in H2? What is the reaction order in NH3? What is overall reaction order? At a certain concentration of H2 and NH3, the initial rate of reaction is 6.0 M / s. What would the initial rate of the reaction be if the concentration of H2 were doubled? Be sure your answer has the correct number of significant digits. M S The rate of the reaction is measured to be 9.0 x 104M/s when [H2] = 1.8 M and [NH3] the rate constant. Be sure your answer has the correct number of significant digits. = 1.6 M. Calculate the value of - 2 - 1 k = |M •S

The rate of a certain reaction is given by the following rate law: rate =k[H,]L] rate =k| H. Use this information to answer the questions below. What is the reaction order in H2? x10 What is the reaction order in I2? What is overall reaction order? At a certain concentration of H2 and I2, the initial rate of reaction is 78.0 M / s. What would the initial rate of the reaction be if the concentration of H2 were halved? Round M S your answer to 3 significant digits. The rate of the reaction is measured to be 0.110 M / s when [H2] = 1.2 M and [I2] = 0.35 M. Calculate the value of the = |M, -1 - 1 •s k = rate constant. Round your answer to 2 significant digits.

Some measurements of the initial rate of a certain reaction are given in the table below. [N₂] [H₂] initial rate of reaction 1.75M 1.94 M 3.00 × 10³ M/s X 1.75M 0.238 M 4.52 × 10³ M/s 5.49M 1.94 M 9.41 × 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 3 significant digits. Also be sure your answer has the correct unit symbol rate = k [₂][₂] = 0 k = 40 20 ロ・ロ X > ?

Please answer all parts.