Be sure to answer all parts.For the decomposition of gaseous dinitrogen pentaoxide,2 N2O5(g) → 4 NO2(g) + O2(g)the rate constant is k = 2.8 × 10¯³ s−1 at 60°C. The initial concentration of N2O5 is 2.31 mol/L.(a) What is [N2O5] after 5.00 min?molL(b) What fraction of the N2O5 has decomposed after 5.00 min?X

Given: k=2.8x10−3s−1;[N2O5]0=2.31mol/L;t=5.00minStep 1: Write the integrated rate…

Answered: Be sure to answer all parts. For the…

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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Consider this reaction: 2H, РО, (ад) — Р,0; (аq)+3н,0 (ад) At a certain temperature it obeys this rate law. = (0.749 M ¿PO, •S Suppose a vessel contains H,PO, at a concentration of 0.660M. Calculate how long it takes for the concentration of H,PO, to decrease by 83.0%. You may 4 assume no other reaction is important. Round your answer to 2 significant digits. S ?
The first order rate constant for the decomposition of N205, according to the reaction: 2 N2O5(g) -> 4 NO2(g) + O2(g) at 70°C is 6.82 x 103 s. Suppose we start with 0.0250 moles of N,Os(g) in a volume of 2.0L. a) How many moles of N2O5 will remain after 5.0 min? b) How many minutes will it take for the quantity of N2Os to drop to 0.010 moles? c) What is the half-life of N,Os at 70°C
7.) The results of kinetics experiments have shown the rate of the following reaction:A + 2B + C ↓ products has the following rate law: rate = k[A]2[B]0[C]1with a rate constant of k = 1.3 × 10–4 L2/mole2·s (M –2·s–1).a.) What is the initial reaction rate if the initial concentrations of A, B, and C, are 0.2, 0.3, and 0.4 M, respectively?b.) What is the initial reaction rate if the initial concentrations of A, B, and C, are 0.2, 2.7, and 0.4 M, respectively?
Consider the reaction below at 100oC T2U (g) ⟶⟶ 2 T (g) + U (g) When [T2U] = 0.250 M, the reaction rate is 9.30 x 10-3 M/s, and when [T2U]o = 0.144 M, the reaction rate is 3.09 x 10-3 M/s, which is the numerical value of the specific-rate constant, k, for this reaction? A. 0.149 B. 0.0372 C. 0.0667 D. 0.250
Consider the following reaction in aqueous solution:5Br−(??) + BrO3−(??) + 6H+(??) ⟶ 3Br2(??)+3H2O(l) If the rate of disappearance of Br–(aq) at a particular moment during the reaction is 0.02 mol L−1 s−1, what is the rate of appearance of Br2(aq) at that moment?
6. The gas phase reaction A+B C has a reaction rate which is experimentally observed to follow the relationship rate= k[A]2[B]. Which one of the following would affect the value of the specific rate constant, k? (a) increasing the temperature(b) changing the concentration of A (c) changing the concentration of B(d) changing the concentration of C (e) all of the above
Consider the following reaction: 5Br (ag) + BrO;¯(aq) + 6H*(aq) → 3Br,(aq) + 3H,O() If the rate of disappearance of Br(ag) at a particular moment during the reaction is 3.5×10 mol L-1s-1, what is the rate of disappearance of BrO (aq) at that moment? O 5.8x 10 mol Ls? 07.0x 10 mol Ls! 0 3.5x 10 mol Lis
The iodide ion reacts with hypochlorite ion (the activeingredient in chlorine bleaches) in the following way:OCl - + I - ----->OI - + Cl - . This rapid reaction givesthe following rate data: (a) Write the rate law for this reaction. (b) Calculate therate constant with proper units. (c) Calculate the ratewhen [OCl-] = 2.0 x 10-3 M and [I - ]= 5.0 x10 - 4 M.
The decomposition of sulfuryl chloride (S0₂Cl₂) is a first-order process. The rate constant for the decomposition at 660 K is 4.5 x 102 ¹ (a) If we begin with an initial 50₂Cl₂ pressure of 335 torr, what is the pressure of this substance after 76 s? torr (b) At what time will the pressure of 50₂Cl₂ decline to one fourth its initial value? By what factor will the pressure of sulfuryl chloride decrease after 4 half lives? Note: The answer wants this value: (335 torr)/value final pressure after decay value
The reaction 2 NO(g) + O2(g) --> 2 NO2(g) proceeds through the following mechanism: 2 NO(g) --> N2O2(g)N2O2(g) + O2(g) --> 2 NO2(g) (a) The second step of this mechanism is rate-determining (slow). What is the rate law for this reaction? Rate = k [NO] [O2] Rate = k [NO]2 [O2] Rate = k [NO] [O2]2 Rate = k [NO]1/2 [O2] Rate = k [NO] [O2]1/2 Rate = k [NO]2 Rate = k [NO]2 [O2]1/2 (b) What would the rate law be if the first step of this mechanism were rate-determining? Rate = k [NO] [O2] Rate = k [NO]2 [O2] Rate = k [NO] [O2]2 Rate = k [NO]1/2 [O2] Rate = k [NO] [O2]1/2 Rate = k [NO]2 Rate = k [NO]2 [O2]1/2 Rate = k [NO]
H2 reacts with ClF. Someone thinks this is the mechanism: H2(g) + ClF(g) → HCl(g) + HF(g) HCl(g) + ClF(g) → Cl2(g) + HF(g) (a) Write the balanced equation for the overall reaction. (b) Identify any intermediates in the mechanism, if any. (c) identify and catalysts in the mechanism, if any. (d) Write rate laws for each elementary reaction in the mechanism. (e) If the first step is slow and the second one is fast, what rate law do you expect to be observed for the overall reaction?
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.

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