PLS HELPGhoursCThe catalyzed decomposition of ethanol at 325°C has a rate constant of 4.00 x 105 L mol ¹s ¹. A graph of the reciprocal of ethanolconcentration versus time gives a straight line. The chemical equation for the reaction at this temperature isC₂H₂OH(g C₂H.(g) + H₂O(g)If the initial concentration of ethanol is 0.024 mol L¹, how long will it take for the pressure to reach 1.4 atm at 325°C?

It will take 0.0315hr for the pressure to reach 1.4atm at 325°C.Explanation:Step 1:Given:•Rate…

Answered: PLS HELP G hours C The catalyzed…

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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Potentially Useful Reference Information -Ea J R = 8.314 k = A· e RT mol·K Calculate the rate constant (k) for a reaction where a 0.1 M first order reactant and a 0.3 M second order reactant result in a rate of 4.5 x 103 M/sec. Report your answer with one significant figure; you do not need to include any units, just the value of k. The molarities given are the initial concentrations for each reactant.
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?
Which of the following statements about rate laws is FALSE? A) Rate laws can only be determined experimentally. B) Rate laws tell us information about the mechanism of the chemical reaction under study. C) The rate law for the chemical reaction A + B + 20 –D must be rate = k[A][B][C]² %3D D)A rate law can only be written for the elementary reactions of a given chemical reaction.
Q3
Consider this reaction: 2NH, (g) - N2 (g) +3H, (g) At a certain temperature it obeys this rate law. rate =(0.0103 s")[NH,] S Suppose a vessel contains NH, at a concentration of 0.170M. Calculate the concentration of NH, in the vessel 68.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. OM x10
Consider the following reaction: A + B + C → D The rate law for this reaction is as follows: [A][C]* Rate = k [B]L/2 Suppose the rate of the reaction at certain initial concentrations of A, B, and C is 1.17x10-2 mol · L-ls¬1. Part A What is the rate of the reaction if the concentrations of A and C are doubled and the concentration of B is tripled? Templates Symbols uado redo reset keyboard shortcuts help Rate = mol · L-!s-1
Consider the reaction described by the equation C,H,Br, (aq) + 3 I (aq) C,H, (g) + 2 Br¯(aq) + I5 (aq) The rate law is rate = k[C,H¸Br,][I¯] where k = 0.00504 M-1. s-1. What are the missing entries in the table? Run [C,H,Br,h (M). [I¯], (M) Initial rate of formation of C,H, (M-s) 1 0.162 0.000529 0.162 y 0.000265 3 0.162 0.162 M X = M y = z = M-s-1
Write the rate law for the following reaction, which represents an elementary step in a reaction. Your rate law should not include the states of matter. so,Cl, (g) · SO2(g) + Cl, (g)
Consider this reaction: 2H1 (g) → H₂(g) +1₂(e) At a certain temperature it obeys this rate law. rate = (0.345-¹) [HI] Suppose a vessel contains HI at a concentration of 0.730M. Calculate how long it takes for the concentration of HI to decrease by 86.0%. You may assume no other reaction is important. Round your answer to 2 significant digits. 0. 08
The reaction CH3NC → CH3CN has a rate constant of 0.498 s-1 at a specific temperature. What is the concentration of CH3NC after 41 seconds if its initial concentration is 1.368 M? (the answer should be entered with 3 significant figures; do not enter units; give answer in scientific notation--valid notation examples include 1.23e-8 and 1.23e8 and -1.23e-4 and 1.23e0) esc 3 7 delete Q E Y P A D G K return ock V B N M command option control option command 10 40 an the a greates4
Consider the following rate law: Rate = k[B] Which of the following equations could be used to find the concentration of B at some time (t) in the reaction? A) [B] = [B]₀ - kt B) [B] = [B]₀ × e^(-kt) C) 1/[B] = 1/[B]₀ + 2kt D) All of the above
considering the balanced equation: 2 N2H4 + N2O4 --> 3N2 + 4 H2O Write the rate law for the dependence of the rate on concentration of the reactants, leaving the experimentally determined values as symbols: rate=K [ ]n etc

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