**Questions:**1. The reaction: 2 NO(g) + 2 H₂(g) → N₂(g) + 2 H₂O(g) produced the following initial rate data for a series of experiments. Use the data to determine the rate law for the reaction. (Show work.)| Expt. | [NO] | [H₂] | Rate, M/sec ||-------|------|-------|-------------|| 1 | 0.0020 | 0.0010 | 0.12 || 2 | 0.0040 | 0.0010 | 0.48 || 3 | 0.0040 | 0.0020 | 0.96 |Rate = ______Calculate the rate constant, k, for the reaction above. (Show work, include units on k.)k = ______

To solve this problem first we have to consider a rate law then we will calculate the order of…

Questions: 1. The reaction: 2 NO(g) + 2 H2(g) N2(g) + 2 H20(g) produced the following initial rate data for a series of experiments. Use the data to determine the rate law for the reaction. (Show work.) Expt. NO] [H2] Rate, M/sec 1 0.0020 0.0010 0.12 0.0040 0.0010 0.48 3 0.0040 0.0020 0.96 Rate = Calculate the rate constant, k, for the reaction above. (Show work, include units on k.) k =

Questions: 1. The reaction: 2 NO(g) + 2 H2(g) N2(g) + 2 H20(g) produced the following initial rate data for a series of experiments. Use the data to determine the rate law for the reaction. (Show work.) Expt. NO] [H2] Rate, M/sec 1 0.0020 0.0010 0.12 0.0040 0.0010 0.48 3 0.0040 0.0020 0.96 Rate = Calculate the rate constant, k, for the reaction above. (Show work, include units on k.) k =

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Part A Consider a simple reaction in which a reactant A forms products: A→products What is the rate law if the reaction is zero order with respect to A? First order? Second order? For each case, explain how a doubling of the concentration of A would affect the rate of reaction. Drag the appropriate items to their respective bins. Reset Help doubling the concentration of A does nothing to the reaction rate Rate = k[A]° = k doubling the concentration of A doubles the reaction rate doubling the concentration of A quadruples the reaction rate Rate = k[A]' = k[A] Rate = k[A]? A zero order reaction A first order reaction A second order reaction
Question 1 Using the data below, report the exponent for each reactant in the rate law, as well as the overall reaction order. rate = k[A}*{B]Y 2A + B- 3C (A] (B] Rate M s-1 0.25 0.10 0.20 0.10 0.40 0.25 0.20 0.50 3 0.80 A.0 B. 1 v y= C.2 v overall reaction order D. 3 E. 4 F. 5 G.6 H.Cannot be determined from the information given AMoving to another question will save this response. MacB 828 F7 F10 2 3 4. 5 8 Q E T Y P { D K L mand alt command option
11. The graph here shows the concentration of reagent A in a reaction. Which is the best estimate of the initial rate of the reaction? Concentration of A (moles/L) vs Time a) 625 M/s 1.000 b) 16.4 M/s 0,900 c) 0.029 M/s 0.800 0.700 d) 7.40 x 10³ M/s 0.600 0.500 0.400 0.300 0.200 0.100 0.000 60 80 0 20 40 time(s) 100 120
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The rate of a certain reaction is given by the following rate law: k[NJ[0] rate = k 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 N, and 03, the initial rate of M reaction is 58.0 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 0.910 M / s when [N2] = 0.29 M and [O3] = 1.4 M. Calculate the value of the -3 - 1 k = rate constant. Round your answer to 2 significant digits.
2) Can some one explain the question
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
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
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Please show all steps in the question attached, right answer 1,1