1. Nitrogen monoxide, NO, reacts with hydrogen to give nitrous oxide, N₂O2, and water, as illustrated in the reaction below. 2NO(g) + H2 (g) →N₂O2 (aq) + H₂O(g) To obtain the rate law for this reaction, the following experiments were run and. for each, the initial rate of the reaction of N₂O2 was determined. What is the value of the rate constant? Exp 1 Exp 2 Exp 3 Initial concentrations H₂ 0.155 M 0.155 M 0.465 M NO 0.327 M 0.109 M 0.109 M N₂O2 Initial Rate 1.9691 M/s 0.0729 M/s 0.0733 M/s

1. Nitrogen monoxide, NO, reacts with hydrogen to give nitrous oxide, N₂O2, and water, as illustrated in the reaction below. 2NO(g) + H2 (g) →N₂O2 (aq) + H₂O(g) To obtain the rate law for this reaction, the following experiments were run and. for each, the initial rate of the reaction of N₂O2 was determined. What is the value of the rate constant? Exp 1 Exp 2 Exp 3 Initial concentrations H₂ 0.155 M 0.155 M 0.465 M NO 0.327 M 0.109 M 0.109 M N₂O2 Initial Rate 1.9691 M/s 0.0729 M/s 0.0733 M/s

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...

See similar textbooks

Similar questions

The reaction between N2O5 and water$$N2O5(g)+H2O(g)2HNO3(g)is a source of nitric acid in the atmosphere. The reaction is first order in each reactant. Write the rate law for the reaction.
Consider following reaction: 2 A2B5(g) → 4AB2(g) + B2(g) The rate constant is 0.129 s-1 at 298 K for this reaction. What is the percent of A2B5 left after the first 19.091 s? Report your answer with three decimals. Enter numbers only;
The isomerization of cyclopropane, C3H6, is believed to occur by the mechanism shown in the equations above. Here C3H6* is an excited cyclopropane molecule. At low pressure, Step 1 is much slower than Step 2. Derive the rate law for this mechanism at low pressure?
consider the reaction 2 H2 (g) + O2 (g) = 2H2O (g). Determine the rate in which H2O is formed
A possible reaction for the degradation of the pesticide DDT to a less harmful compound was simulated in the laboratory. The reaction was found to be first order, with k = 2.55 x 108 s at 25°C. What is the half-life for the degradation of DDT in this experiment, in years? (1 year = 365 days) Round your answer to 2 decimal places.
Consider this reaction: 2SO3 (g) →2SO₂(g) + O₂(g) At a certain temperature it obeys this rate law. rate = (0.894 M¹-s¹) [S0₂] Suppose a vessel contains SO3 at a concentration of 0.390 M. Calculate the concentration of SO3 in the vessel 8.60 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M Explanation Check 0 10 Q Search a Ⓒ2023 McGraw Hill LLC. All Rights Reserved. Terms of Use O Privacy Center
3. Consider the reaction below: 2NO (g) + Cl,(g)'n 2NOCI (g) A mechanism involving these steps has been proposed for the reaction: Step 1: NO (g) + Cl,(g)'n NOCI, (g) Step 2: NOCI, (g) + NO(g)'n 2NOCI (g) The rate law for the reaction is given by rate = k[NO][Cl]. (a) What is the reaction intermediate? (b) Which is the rate-determining step? (c) Is the rate-determining step unimolecular, bimolecular, or termolecular? Why?
Consider the reaction 5Br−(aq)+BrO−3(aq)+6H+(aq)→3Br2(aq)+3H2O(l) The average rate of consumption of Br− is 1.26×10−4 M/s over the first two minutes. What is the average rate of formation of Br2 during the same time interval?
Consider the reaction for the formation of ammonia, NH3: N2(g) + 3 H2(g) --> 2 NH3(g) Which is the correct rate expression for this reaction?
Consider this reaction: 2SO3 (g) →2SO₂ (g) + 0₂ (8) At a certain temperature it obeys this rate law. rate= (0.00626 s¹)[03] Suppose a vessel contains SO3 at a concentration of 0.250M. Calculate the concentration of SO3 in the vessel 99.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 X Ś