Nitrosyl chloride, NOCl, decomposes to NO and Cl2. Determine the rate constant for this reaction from the following data:   [NOCl] (M) 0.10 0.20 0.30 Rate (mol L–1 h–1) 8.0x10–10 3.2 x10–9 7.2x10–9   Group of answer choices A, 8.0x10–7 B, 8.0x10–8 C, 8.0x10–9 D 8.0x10–6

A chemistry graduate student is studying the rate of this reaction: 2SO3 (g) 2So, (g) +0, (g) He fills a reaction vessel with SO, and measures its concentration as the reaction proceeds: time [so,] olo (seconds) 18 0.200M Ar 0.10 0.127M 0.20 0.0805 M 0.30 0.0511 M 0.40 0.0324M Use this data to answer the following questions. Write the rate law for this reaction. rate = k|| x10 Calculate the value of the rate constant k.

Consider this reaction: NH,OH (аq) — NH, (ад)+ н,о (ад) At a certain temperature it obeys this rate law. rate = (0.619 s)[NH,OH] S Suppose a vessel contains NH,OH at a concentration of 0.340M. Calculate the concentration of NH,OH in the vessel 2.60 seconds later. You may assume no 4 other reaction is important. Round your answer to 2 significant digits. ) M x10

R=K [A] [B] ----; 2. The initial rate of the reaction: BrO3(aq) + 5 Br (aq) + 8 H*(aq) Has been measured at the reactant concentrations shown (in mol/L): Trial [BrO3] [Br] [H*] 1 0.10 0.10 0.10 2 0.20 0.10 0.10 3 0.10 0.20 0.10 4 0.10 0.10 0.20 A) Determine the rate law equation including the k value. Determine the order of reaction for BrO3, Br, and H* Rate law 3 Br₂(l) + H₂O(l) Initial rate (mol/Ls) 8.0 x 104 1.6 x 10³ 1.6 x 10°³ 3.2 x 10'³

Some measurements of the initial rate of a certain reaction are given in the table below. H2||2| initial rate of reaction 0.554M| 1.43M 2.00 M/s 1.05 M 1.43 М 3.79 M/s 0.554M 4.76M 6.66 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 I x10 k =

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

The reaction 4 HBr(g) + O2(g)  2 H2O(g) + 2 Br2(g) was studied at a certain temperature with the following results:   Experiment [HBr(g)] (M) [O2(g)] (M) Rate (M/s)   1 0.00542 0.00542 0.341 2 0.00542 0.0108 0.679 3 0.0108 0.00542 0.679 4 0.0108 0.0108 1.35 (a) What is the rate law for this reaction? Rate = k [HBr(g)] [O2(g)] Rate = k [HBr(g)]2 [O2(g)]     Rate = k [HBr(g)] [O2(g)]2 Rate = k [HBr(g)]2 [O2(g)]2 Rate = k [HBr(g)] [O2(g)]3 Rate = k [HBr(g)]4 [O2(g)] (b) What is the value of the rate constant? (c) What is the reaction rate when the concentration of HBr(g) is 0.00861 M and that of O2(g) is 0.0123 M if the temperature is the same as that used to obtain the data shown above? _________M/s

Write a balanced reaction for which the following rate relationships are true. Rate (A[NO]/At) = - (1/2)(A[HNO3]/At) = (A[H₂O]/At) = (1/3)(A[NO₂]/At) No +해 + + HNO3 H₂O 1 NO₂ 6 NO3HNO3 6H 20 + 2NO₂ If the rate of disappearance of NO in the reaction in #1 is 0.270 M s-1 at 150°C, the rate of appearance of NO3 is. What is the overall order of the reaction in #1, if given is the rate law? Rate = k[NO]2 [HNO3]³ Ms-1 Given the above rate law, how does the rate of reaction change if the concentration HNO3 is doubled? ANSWER:

Initial-rate data at a certain temperature is given in the table for the reaction SO₂Cl₂(g) → SO₂(g) + Cl₂ (g) [SO₂Cl₂], (M) k = 0.100 0.200 0.300 Initial rate (M/s) 2.40 x 10-6 4.80 x 10-6 7.20 x 10-6 Determine the value and units of the rate constant. units:

Consider this reaction: →H2CO3aq+H2OaqCO2aq At a certain temperature it obeys this rate law.rate =·0.0579M−1s−1H2CO32 Suppose a vessel contains H2CO3 at a concentration of 0.820M. Calculate the concentration of H2CO3 in the vessel 280.seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. =___M