Show all work. Include any equations used, substitutions, and algebra as needed. Round tosignificant digits.19. A first order reaction starts with an initial concentration of reactant A of 3.00 M and hasa rate constant of 6.31 x10-3 s 1. What is the concentration of the reactant after (a) 10seconds (b) 1 minute and (c) 3 minutes?

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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...

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A reaction is first order with respect to reactant "A" and has a half life of 16 minutes. How long does it take for the concentration of A to drop from 1 g to 1/64 g? 80 mins 96 mins 2 hrs and 32 minutes 16 mins
CHAn experiment is carried out to measure the rate of the reaction, which is first order. A 4.70 x 10-3 mol sample of CH3CH2NH2 is placed in a previously evacuated 2.00 L container at 773 K. After 20.0 minutes, the concentration of the CH3CH2NH2 is found to be 3.60 x 10-4 mol/L. A. Calculate the rate constant for the reaction at 773 K. Include units with your answer. B. Calculate the initial rate, in M*min-1 , of the reaction at 773 K.
Suppose you have a reaction between A and that forms product C: A B C and that A and B are both added at equal concentrations to a reaction vessel. At the end of 120 min you find that the concentration of A is just 30% of what it was originally. You have previously determined that the reaction proceeds as first order in [A] and zero order in [B]. How much of the initial amount of A will remain at the end of 240 min? 9.00 % O 17.6% O 0.000% O 14.2%
At a certain temperature this reaction follows first-order kinetics with a rate constant of 0.0654 s 2NH₂(g) →1 → N₂(g) + 3H₂(g) Suppose a vessel contains NH3 at a concentration of 0.680M. Calculate the concentration of NH3 in the vessel 9.20 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M 0.0 X S
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Smail ||| YouTube O KINETICS AND EQUILIBRIUM Using an integrated rate law for a first-order reaction At a certain temperature the rate of this reaction is first order in NH4OH with a rate constant of 0.0108 s NH,OH(aq). } → NH, (aq) +H,O(aq) Translate M Suppose a vessel contains NH4OH at a concentration of 1.24 M. Calculate the concentration of NH OH in the vessel 63.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. Explanation 82°F Mostly cloudy Check 0/5 Q Search © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | 1
The graph below depicts the consumption of reactant A during a first-order reaction. (Enter all values to two significant figures.) [A], (M) 0.3 0.25 0.2 0.15 0.1 0.05 5 10 15 20 25 30 35 40 45 50 55 60 65 Using the graph, determine the half-life of the reaction. S (b) Calculate the rate constant and its units. ??? Time (s) Submit Answer
F8 =9 =10 = 11 = 12 = 13 14 = 15 16 18 19 At a certain temperature this reaction follows second-order kinetics with a rate constant of 0.0618M-¹.s-¹: 2NH3 (g) → N₂ (g) + 3H₂ (g) Suppose a vessel contains NH3 at a concentration of 1.25 M. Calculate the concentration of NH3 in the vessel 68.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. OM ? Su ontinue 0 10 X S hp
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What are the reaction orders with respect to A, B, and C, respectively?A) 0, 1, 1B) 1, 2, 1C) 1, 1, 1D) 1, 2, 0E) 0, 2, 1
A first-order reaction has a rate constant of 3.6 x 10-3s-1. How many seconds does it take for the reaction to be 31.3% complete? (Report an integer)

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