• Part A The specific rate constant for the first-order decomposition of N2O5 (g) to NO2(9) and Oz(9) is 7.48 x 10s at a given temperature. Find the length of time required for the total pressure in a system containing N2Os at an initial pressure of 0.110 atm to rise to 0.155 atm. Express your answer using two significant figures. VO AE ? t = 230 Submit Previous Answers Request Answer X Incorrect; Try Again; 3 attempts remaining Part B Find the length of time required for the total pressure in a system containing N2O5 at an initial pressure of 0.110 atm to rise to 0.210 atm. Express your answer using two significant figures. ? t = Submit Request Answer • Part C Find the total pressure after 100 s of reaction. Vol AE ? P = atm Submit Request Answer

• Part A The specific rate constant for the first-order decomposition of N2O5 (g) to NO2(9) and Oz(9) is 7.48 x 10s at a given temperature. Find the length of time required for the total pressure in a system containing N2Os at an initial pressure of 0.110 atm to rise to 0.155 atm. Express your answer using two significant figures. VO AE ? t = 230 Submit Previous Answers Request Answer X Incorrect; Try Again; 3 attempts remaining Part B Find the length of time required for the total pressure in a system containing N2O5 at an initial pressure of 0.110 atm to rise to 0.210 atm. Express your answer using two significant figures. ? t = Submit Request Answer • Part C Find the total pressure after 100 s of reaction. Vol AE ? P = atm Submit Request Answer

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

Please show all work!
a) A chemical reaction is given below. Write the rate of the reaction with respect to each reactant and product. CH3 + 50, → 3Co, + 4H,0 b) A Kinetic experiment gives the following data for the following reaction. Find the average rate of the reaction between t=0 sec to t=15 sec and also between t= 5 sec and t-20 sec. OCr +r → Ol + Cr [ OCr ]M 1.2 0.8 0.3 0.6 0.4 t (sec) 0 5 10 15 20
Cindy decomposed a metal hydroxide via the reation: Mt(OH) 3 → MtO + H20, and then collected concentration and time data. After analyzing on her TI84 the following data were obtained. [Mt(OH)3] vs. time a = 2.10 x 104 In[Mt(OH)3] vs. time a = -5.80 x 10-5 b = -0.770 r = 0.999 [Mt(OH)3] vs. time a = -1.72 x 10-5 b = 0.450 r = 0.917 2.00 %3D r² 0.981 What is the order with respect to Mt(OH)3? What is the value of the rate constant for this reaction?
At a certain temperature this reaction follows first-order kinetics with a rate constant of 0.0667 s¯¹: NH,OH (aq) → NH, (aq)+H,O (aq) Suppose a vessel contains NH4OH at a concentration of 0.360M. Calculate the concentration of NH4OH in the vessel 15.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 X ?
2NO(g) +O2(g) → 2NO(g) The following kinetic data were obtained for the initial rates of disappearance of NO: Expriment Initial Conc. of NO Initial Conc. of O2 Initial Rate Exp. 1 0.0125 M 0.0253 M 0.0281 M/s Exp. 2 0.0250 M 0.0253 M 0.112 M/s Exp. 3 0.0125 M 0.0506 M 0.0561 M/s What is the value of the rate constant for the reaction? Express your answer to three significant figures. Just enter the number (e.g. 2.48x10^-4) and the unit.
Hi! Please use the graph in the question to answer part a!
a) A chemical reaction is given below. Write the rate of the reaction with respect to each reactant and product. [2 Marks] 2C2H6 +702-→ 4CO, + 6H2C b) A Kinetic experiment gives the following data for the following reaction. Find the average rate of the reaction between t-5 sec to t-15 sec and also between t= 15 sec and t=20 sec. [2 Marks] OC + 1 OI + CI 1.2. 08 0.6 0.4 0.3 t (sec) 10 15 20 A- BI 12:29 A D 7 ) ENG 4/11/4
QUESTION 1 The thermal decomposition of an oxide produced the following data: time (5) 120 180 240 300 560 680 [oxide] (M) 1.2 0.53 0.41 0.34 0.29 0.17 0.15 0.00 Determine: a) The order of the reaction. Explain your reasoning. b) The rate constant of the reaction. Be sure to include units and explain how you arrived at this answer.
Question 30 of 39 Submit The zero order reaction A → Products takes 63.5 minutes for the concentration of A to decrease from 0.970 M to 0.205 M. What is the value of k for this reaction? M/min 1 3 4 C 7 8 9 +/- х 100 Tap here or pull up for additional resources
At a certain temperature this reaction follows second-order kinetics with a rate constant of 64.6M¹s¹: NH,OH(aq) → NH, (aq)+H,O(aq) Suppose a vessel contains NH OH at a concentration of 0.170M. Calculate the concentration of NH OH in the vessel 0.920 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. 0 M x10 X S 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center 1 Accessibility Show All
Consider a first order reaction AB }A+ B If the reaction is 34% complete at the end of 39 s, what is the length of the half-life of this reaction in seconds? Use 2 significant figures in your answer. Do not include the unit.
A certain reaction is second order in N₂ and first order in H₂. Use this information to complete the table below. Be sure each of your answer entries has the correct number of significant digits. 1.58 M 0.540 M 3.89 M 0.382 M 0.382 M 0.155 M Explanation initial rate of reaction Check 0.440 M/s Mis MIS X S tv W MacBook Air © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center C 5 Accessibility