Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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- The reaction described by the equation 0,(g) + NO(g) → 0,(g) + NO,(g) has, at 310 K, the rate law rate of reaction = k[O,][NO] k = 3.0 × 106 M-!·s-! Given that [O,] = 4.0 × 10-4 M and [NO] = 2.0 × 10-³ M at t = 0, calculate the rate of the reaction at t = 0. %3D rate: M/s What is the overall order of this reaction? 3arrow_forwardFor the reaction AB(g) —>A(g) + B(g) the rate law is determined to be rate =k[AB]^2 and k=0.255 L/mol-min. If the initial concentration of AB is 1.00M, how long will it take for the concentration of AB to fall to 0.40M?arrow_forwardSome measurements of the initial rate of a certain reaction are given in the table below. [N] 0.815M1.56M N,|H||initial rate of reaction 185. M/s 141.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. 口 rate = 0 ロ || = 1 Explanation Check D2022 McGrny Hl LLC. Al Rights Reserved. Terms of N 回 至 五arrow_forward
- Which of the following statements about rate laws is FALSE? A) Rate laws can only be determined experimentally. B) Rate laws tell us information about the mechanism of the chemical reaction under study. C) The rate law for the chemical reaction A + B + 20 –D must be rate = k[A][B][C]² %3D D)A rate law can only be written for the elementary reactions of a given chemical reaction.arrow_forwardConsider the hypothetical reaction: A + B + 2C → 2D + E where the rate law is Rate = -ALA) = k[A][B]2 An experiment is carried out where [Alo = 7.200 x 102 M, [B]. = 2.500 M and [Cla = 2.500 M. The reaction is started, and after 11.60 seconds, the concentration of A is 2.200 x 10° M. Calculate the value of k for this reaction in units of M2s1. Answer:arrow_forwardConsider this reaction: 2HI (g) → H, (g) +I, (g) At a certain temperature it obeys this rate law. rate =(0,465 s)[HI Suppose a vessel contains HI at a concentration of 0.540M. Calculate the concentration of HI in the vessel 2.80 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits.arrow_forward
- A reaction proceeds according to the following equation: A + 3B → 2C + 2D At an early stage of the reaction, conc. A = 1.991 M and 5.23 minutes later, conc. A= 0.861 M. What is the average rate of the reaction during this time period, expressed in units of M·s-1? Report your answer with four decimals. Enter numbers only; do not enter units.arrow_forwardThe rate of a certain reaction is given by the following rate law: rate = k[N,][H] Use this information to answer the questions below.arrow_forwardConsider this reaction: CICH, CH, CI (g) → CH,CHCI (g) +HC1 (g) At a certain temperature it obeys this rate law. rate = (0.0361 s")[CICH,CH,CI] Suppose a vessel contains CICH,CH,Cl at a concentration of 0.860M. Calculate the concentration of CICH,CH,Cl in the vessel 36.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits.arrow_forward
- Write the rate law for the following reaction, which represents an elementary step in a reaction. Your rate law should not include the states of matter. so,Cl, (g) · SO2(g) + Cl, (g)arrow_forwardOzone reacts with nitrogen dioxide to produce oxygen and dinitrogen pentoxide according to the following chemical equation: O3(g) + 2NO2(g)→ 02(g) + N2O5(g) The rate law for this reaction is Rate = k[O3]|NO2]. If concentration is measured in moles per liter and time is measured in seconds, what are the units of k?arrow_forwardConsider this reaction: 2H1 (g) → H₂(g) +1₂(e) At a certain temperature it obeys this rate law. rate = (0.345-¹) [HI] Suppose a vessel contains HI at a concentration of 0.730M. Calculate how long it takes for the concentration of HI to decrease by 86.0%. You may assume no other reaction is important. Round your answer to 2 significant digits. 0. 08arrow_forward
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