The reaction between A and B in dilute aqueous acidic solution is: 2H2(g) + 2NO(g) N2{g) + 2H2O(g) If the collected data for each reactant (M) vs. initial rate (M s) are in the table, what is the rate law? [NO] [H2] Rate 0.10 0.10 2.0x102 0.20 0.20 16x102 0.10 0.20 4.0x10-2 O rate = k[NO]²[H2] O rate = k[NO][H2]? rate = k[NO]°[H2]² O rate = k[NO]? [H2]²/[N>][H2O]?

2. At 325°C, N0,(g) reacts with CO(g) to yield NO(g) and CO,(g). The reaction is: NO,(g) + CO(g) I NO(g) + CO,(g) It is observed that the reaction rate does not depend upon the concentration of CO, and t\so the reaction rate law does not involve [CO]. The rate does depend upon [NO,], however, and the following data is obtained. Determine the rate law and the value of the rate constant. Rate ( M sec ') NO,] 1. 1 X 10 -2 0.15 4.5 X 10-2 0.3 1.8 X 10- 4.0 X 10-13 0.6 0.9

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 > ?

Find the rate constant (k)

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Consider this reaction: 2N₂O5 (g) → 2N₂O4 (g) + O₂(g) At a certain temperature it obeys this rate law. = (0.291 M¹s¹) [N₂0₂] rate Suppose a vessel contains N₂O, at a concentration of 0.230 M. Calculate how long it takes for the concentration of N₂O to decrease to 23.0% of its initial value. You may assume no other reaction is important. Round your answer to 2 significant digits. ? Subm Continue Ⓒ2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Cente 80°F Partly sunny ^ pe here to search B X G

Consider this reaction: 2N₂O5 (g) → 2N₂O4 (g) + O₂(g) At a certain temperature it obeys this rate law. rate = (0.0317 M¹-s¯¹) [₂0₂] S Suppose a vessel contains N₂O5 at a concentration of 0.440 M. Calculate the concentration of N₂O5 in the vessel 480. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 ? X S

26.  Hydrogen reacts with nitrogen monoxide to form dinitrogen monoxide (laughing gas) according to the equation: H2(g)+2NO(g)⟶N2O(g)+H2O(g) Determine the rate law, the rate constant, and the orders with respect to each reactant from the following data: [NO] (M) 0.30 0.60 0.60 [H2] (M) 0.35 0.35 0.70 Rate (mol L−1 s−1) 2.835 × 10−3 1.134 × 10−2 2.268 × 10−2

Consider the fictitious reaction and the rate law below. What is the overall order of the reaction? What happens to the rate of the reaction when the concentration of X stays the same and the concentration of Y doubles? X (g) + Y (g) → XY (g)                     rate = k[X][Y]

The following are initial rate data for: A + 2B - C + 2 D Experiment Initial [A] Initial [B] Initial Rate 1 0.10 0.10 0.300 0.20 0.10 0.600 3 0.10 0.20 1.200 What is the rate law? The rate law is Rate = k[A]?[B]1. The rate law is Rate = k[A]?[B]*. The rate law is Rate = k[A]?[B]°. The rate law is Rate = k[A]°[B]?. The rate law is Rate = k[A]²[B]².