The first-order rate constant for the decomposition of N₂O5, given below, at 70°C is 6.82 x 10-3 s-1. Suppose we start with 0.0500 mol of N₂O5 (g) in a volume of 4.5 L.2 N₂O5(9)→ 4 NO₂(g) + O₂(g)(a) How many moles of N₂O5 will remain after 3.0 min?0.0146mol(b) How many minutes will it take for the quantity of N₂O5 to drop to 0.005 mol?min(c) What is the half-life of N₂O5 at 70°C?min

Given,the decomposition reaction:Initial moles of N2O5 = 0.0500 molThe rate constant = 6.82 x 10-3…

The first-order rate constant for the decomposition of N₂O5, given below, at 70°C is 6.82 x 10 2 N₂05(9)→ 4 NO₂(g) + O₂(g) (a) How many moles of N₂O5 will remain after 3.0 min? 0.0146 mol (b) How many minutes will it take for the quantity of N₂O5 to drop to 0.005 mol? min (c) What is the half-life of N₂O5 at 70°C? min

The first-order rate constant for the decomposition of N₂O5, given below, at 70°C is 6.82 x 10 2 N₂05(9)→ 4 NO₂(g) + O₂(g) (a) How many moles of N₂O5 will remain after 3.0 min? 0.0146 mol (b) How many minutes will it take for the quantity of N₂O5 to drop to 0.005 mol? min (c) What is the half-life of N₂O5 at 70°C? min

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

15.For the reaction, 2H,S(g) + 0,(g) 2S(s) + 2H,0(1), which one of the following statements is absolutely true? (a) The reaction is first order with respect to H,S and second order with respect to O (b) The reaction is fourth order overall. (c) The rate law is: rate = k[H,S][0,]. %3D (d) The rate law is: rate = k[H,S][O,]. %3D (e) The rate law cannot be determined from the information given.
Under certain conditions the rate of this reaction is zero order in dinitrogen monoxide with a rate constant of 0.0088 M:5 2N,0 (g) → 2 N, (g) + 0; (g) Suppose a 400. mL flask is charged under these conditions with 200. mmol of dinitrogen monoxide. After how much time is there only 100. mmol left? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. x10 O
For the decomposition of gaseous dinitrogen pentaoxide, 2 N₂O5(g) → 4 NO₂(g) + O₂(g) the rate constant is k = 2.8 × 10-3 s¹ at 60°C. The initial concentration of N₂O5 is 2.23 mol/L. (a) What is [N₂O5] after 5.00 min? mol L (b) What fraction of the N₂O5 has decomposed after 5.00 min?
The reaction: 2NO2 --> 2NO + O2 has the rate law: Rate = k[NO2]2 When the reaction was carried out at 300oC, it took 1.00 x 102 seconds for [NO2] to decrease from 0.0100 M to 0.0065 mol/L. How long does it take for [NO2] to decrease from 0.0100 M to 0.0050 M? (A) 143 s (B) 158 s (C) 186 s (D) 286 s
Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of 0.0032 M's ¹: → 3H2(g) → 2 NH3 (g) N2(g) +3H₂ (g) Suppose a 450. mL flask is charged under these conditions with 350. mmol of ammonia. How much is left 60. s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.
Consider the reaction: 4 A + 7 B → 4 C + 6 D At a certain instant, the initial rate of disappearance of the reactant B is X. a) What is the initial rate of the appearance of product D at the same instant? [ Select ] b) The average rate of appearance of product D in the reaction is found to be 4.23 x 102 M over a certain interval of time. What is the rate of disappearance of reactant B during this interval? [ Select ] c) Assume that the rate law of the reaction is given by Rate = k{B}. The reaction takes 36 s to consume 25% of reactant B. Calculate the percentage remaining of reactant B after another 80 s in the same reaction. [ Select ]
2N2O (g) —-> 2N2 (g) + O2 (g) a) express the rate of the reaction in terms of the change in concentration of each of the reactant and products. b) In the first 15 seconds of the reaction, 0.015 mol of O2 is produced in a reaction vessel with the volume of 0.500 L. What is the average rate of the reaction during this time interval? c) Predict the rate of change in the concentration of N2O during this time interval. In other words, what is △[N2O]/ △t?
Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of 0.0076 M•s *: 2 NH, (g) → N2 (g) + 3 H, (g) Suppose a 5.0 L flask is charged under these conditions with 500. mmol of ammonia. How much is left 3.0 s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits. x10
The rate constant for the reaction 2N2O5(g) → 4NO2(g) + O2(g) is equal to 3.41 x 10–5 s–1 at 30 ºC. If the initial concentration of N2O5is 0.446 M what concentration of NO2 will be observed after 175 minutes? Assume that initially no NO2 was present in the reaction vessel.
Chlorine dioxide, CIO₂, is a reddish-yellow gas that is soluble in water. In basic solution it gives CIO3 and ClO₂ ions. 2 CIO₂(aq) + 2 OH(aq) → CIO3(aq) + ClO₂ (aq) + H₂O(1) To obtain the rate law for this reaction, the following experiments were run and, for each, the initial rate of reaction of ClO₂ was determined. Use the data here to determine the order of the reaction for CIO₂ and OH, and the value of the rate constant. [CIO2]init [OH Jinit Initial Rate, mol/(Los) Exp. 1 0.030 Exp. 2 0.060 Exp. 3 0.030 Order for CIO₂: Order for OH": Rate constant = 0.030 0.030 0.060 0.0062 0.0248 0.0124
Under certain conditions the rate of this reaction is zero order in hydrogen lodide with a rate constant of 0.0038 M's ': 2 HI(g) H,(g)+1,(g) Suppose a 4.0L flask is charged under these conditions with 100, mmol of hydrogen lodide. After how much time is there only 50.0 mmol left? You may assume no other reaction Is important. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits.
The first-order rate constant for the decomposition of N2O5, 2N2O5(g) yields 4NO2(g) at 70∘C is 6.82 x 10-3 s-1 . Suppose we start with 2.30×10−2 mol of N2O5(g) in a volume of 1.8 L . How many moles of N2O5 will remain after 7.0 minutes?