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. %3D -3 -1 OM k =

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. 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 01/2 S - 2 - 1 = M ² ² ₁8² ¹ •S x10 × Ś

For the multi-step reaction A+B → C+D the rate-limiting step is unimolecular, with A as the sole reactant. If [A] and [B] are both 0.175 M, then the rate of reaction is 0.0030 M/s. What is the rate of the reaction if [A] is doubled? rate: Starting with the original concentrations, what is the rate of the reaction if [B] is halved? rate: Starting with the original concentrations, what is the rate of the reaction if [A] and [B] are both increased by a factor of 5? rate: M/s M/s M/s

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 ☑

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Consider the rate law: Rate = k[NO][O,] Which of the following statements is FALSE regarding this rate law? O The value of k will increase with temperature. O The reaction is 2nd order overall. O The reaction is 1st order with respect to O2 The reaction is 2nd order with respect to NO.

The rate of a certain reaction is given by the following rate law: rate =k| N,| H2 -k[N;][H+]° Use this information to answer the questions below. What is the reaction order in N,? What is the reaction order in H2? What is overall reaction order? At a certain concentration of N, and H2, the initial rate of reaction is 0.620 M / s. What would the initial rate of the reaction be if the concentration of N, were halved? Round M S your answer to 3 significant digits. The rate of the reaction is measured to be 24.0 M / s when [N2] = 1.5 M and [H2] = 0.16 M. Calculate the value of the k = |M -2 -1 •S rate constant. Round your answer to 2 significant digits.

Need help in the last 3

Please solve the entire question - I already know that the reaction order in NO is 2 and the reaction order in O2 is 1 - making the overall reaction order 3.