The rate of a certain reaction is given by the following rate law: rate=k[H₂][1₂] Use this information to answer the questions below. 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 0.020 M/s. What would the initial rate of the reaction be if the concentration of H₂ were doubled? Round your answer to 2 significant digits. The rate of the reaction is measured to be 4.0 x 105 M/s when [H₂] = 0.85 M and [1₂] 1.0 M. Calculate the value of the rate constant. Round your answer to 2 significant digits. 1 k = M 1 2 -1 -1 S

I need help with all parts of this question please.

The rate of a certain reaction is given by the following rate law: rate =k Use this information to answer the questions below. What is the reaction order in N,? What is the reaction order in 03? What is overall reaction order? At a certain concentration of N, and 03, the initial rate of M reaction is 6.0 x 103 M / s. What would the initial rate of the reaction be if the concentration of N, were halved? Round S your answer to 2 significant digits. The rate of the reaction is measured to be 0.870 M / s when = 0.90 M and [03] = 0.15 M. Calculate the value of the k = M -3 -1 [N2] •S rate constant. Round your answer to 2 significant digits.

The rate of a certain reaction is given by the following rate law: rate=k =k[N₂]³[03] Use this information to answer the questions below. What is the reaction 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 74.0 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. The rate the reaction is measured to be 6.0 x 104 M / s when [N₂] = 0.79 M and [03] = 1.7 M. Calculate the value of the rate constant. Be sure your answer has the correct number of significant digits. M 0-%/ S - 3 1 k = | M²³ · s¯¹ S x10 X 5 ?

Using a rate law The rate of a certain reaction is given by the following rate law: rate = k [N2]³ [03] Use this information to answer the questions below. What is the reaction order in N₂? What is the reaction order in O3? What is overall reaction order? At a certain concentration of N2 and O3, the initial rate of reaction is 0.560 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. M ㄧˋ S The rate of the reaction is measured to be 4.0 x 104 M/s. when [N2] = 0.81 M and [03] = 0.67 M. Calculate the value of the rate constant. Round your answer to 2 significant digits. k = | M -3 -1 .S ☐ x10 ☑

Using a rate law The rate of a certain reaction is given by the following rate law: =k[N₂] [H₂]² Use this information to answer the questions below. rate = 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. = k = M -2 1 2 3 01/1/2 • S S – 1 ■ x10 X Ś ? 00. 18 Ar Ò Show all ie... Show all

The rate of a certain reaction is given by the following rate law: rate = k[H₂]²[NH₂] 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 34.0 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 0.040 M/s when [H₂] = 1.3 M and [NH3] = 0.51 M. Calculate the value of the rate constant. Round your answer to 2 significant digits. 0 10 0 k=M M. S - 0M 72-571

The rate of a certain reaction is given by the following rate law: rate = 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 0.240 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 88.0 M/s when [N₂] = 0.55 M and [H₂] = 1.4 M. Calculate the value of the rate constant. Round your answer to 2 significant its. 0 0 7 -2 -1 K = 0M ²²-5²¹ M². k M S

Try Again Your answer is incorrect. • Row 4: Your answer is incorrect. The rate of a certain reaction is given by the following rate law: rate=k[H₂] [¹₂] Use this information to answer the questions below. What is the reaction order in H₂? 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 8.0 x 104 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. = The rate of the reaction is measured to be 83.0 M/s when [H₂] 0.31 M and [1₂] = 1.4 M. Calculate the value of the rate constant. Be sure your answer has the correct number of significant digits. ₁1 — 2 4 M 1.6 × 10 2 k 1.9 X 10 M - 1 S • S - 1

The rate of a certain reaction is given by the following rate law: rate =k[H,]°[NH,] Use this information to answer the questions below. What is the reaction order in H,? x10 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 17.0 M / s. What would the initial rate of the reaction be if the concentration of H, were doubled? Round M your answer to 3 significant digits. The rate of the reaction is measured to be 5.0 x 103 M/s when [H2] = 0.95 M and [NH3] = 0.65 M. Calculate the value -2 -1 k = of the rate constant. Round your answer to 2 significant digits.