Consider the following data for the gas-phase decomposition of NO₂ 2NO₂ (9) 2NO (g) + 0₂ (9) Temperature Initial (K) NO₂ 600 0.0010 0.0020 0.0020 600 700 Initial Rate of Decomposition of NO₂ (M/s) 5.4 x 10-7 2.2 x 10 5.2 x 105 Part A If 5.5x10-³ M of NO₂ is introduced into a 1.0 L flask and allowed to decompose at 680 K, how many seconds does it take for the NO₂ concentration to drop to 1.0×10-³ M? Express your answer using two significant figures. 195| ΑΣΦΑ += 1.5.10³ BI ? Submit Previous Answers Request Answer Review | Constants | Periodic Tab * Incorrect; Try Again; One attempt remaining

Consider the following data for the gas-phase decomposition of NO₂ 2NO₂ (9) 2NO (g) + 0₂ (9) Temperature Initial (K) NO₂ 600 0.0010 0.0020 0.0020 600 700 Initial Rate of Decomposition of NO₂ (M/s) 5.4 x 10-7 2.2 x 10 5.2 x 105 Part A If 5.5x10-³ M of NO₂ is introduced into a 1.0 L flask and allowed to decompose at 680 K, how many seconds does it take for the NO₂ concentration to drop to 1.0×10-³ M? Express your answer using two significant figures. 195| ΑΣΦΑ += 1.5.10³ BI ? Submit Previous Answers Request Answer Review | Constants | Periodic Tab * Incorrect; Try Again; One attempt remaining

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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= ○ KINETICS AND EQUILIBRIUM Expressing the concentration of an intermediate in terms of the... Consider the following elementary reaction: CFC1₂(g) → CFC1₂(g) +C1(g) Suppose we let k₁ stand for the rate constant of this reaction, and k_₁ stand for the rate constant of the reverse reaction. 1 Write an expression that gives the equilibrium concentration of CFC1, in terms of k₁, k₁, and the equilibrium concentrations of CFC13 and C1. 1' [CFC₁₂] = 0 √6 X 5 0/5
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40.Consider the following reaction: N2 (g) + 3H2 (g) → 2NH3 (g) if N2 disappears at 0.20 M/min, at what rate is H2 disappearing? Group of answer choices 0.2 0.60 0.1 3
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Part A Consider the following data for the gas-phase decomposition of NO2: 2NO2 (g) → 2NO (g) + O2 (g) If 5.5×10-3 M of NO2 is introduced into a 1.0 L flask and allowed to decompose at 670 K , how many seconds does it take for the NO2 concentration to drop to 1.0x10-3 M ? Initial Rate of Decomposition of Temperature (K) Initial [NO2] NO2 (M/s) Express your answer using two significant figures. 600 0.0010 5.4 x 10-7 600 0.0020 2.2 x 10–6 ? -5 700 0.0020 5.2 x 10 %3D S Submit Previous Answers Request Answer
Determine the rate law and the value of k for the following reaction using the data provided. 2 N205(g) 4 NO2(8) + O2(8) N205h (M) Initial Rate (M/s) 0.093 4.84 x 10-4 0.174 9.05 x 10-4 0.224 1.16 x 10-3 Rate = 6.0 x 10-1 M-25-1[N20513 Rate = 1.6 x 10-3 M1/25-1[N205]1/2 Rate = 5.2 x 10-3 s[N205] Rate = 1.7 x 10-2 M1/2s-1[N205]3/2 Rate = 5.6 x 10-2 M-151IN20512
Write the rate law for the decomposition of ammonium nitrite into nitrogen gas and water using the following data. NH4+1, Taq) + NO2(aq) → N2{g) + 2H2O) Trial [NH4*4]; [NO24}; Rate (M/s) 1 0.010 0.20 5.4x107 0.020 0.20 10.8x107 0.20 0.020 10.8x107 4 0.20 0.040 21.6x10-7 rate = 0.0027 M-1.5-1[NH4*+][NO21] rate = 0.000031s[NH4*1] rate = 0.0000012 s1[NH4*1] rate = 0.000029 s[NO21] O rate = 0.0000012 M-1.s1[NH4*1][NO24] O rate = 0.0000012 s1[NO24]
Chlorine dioxide (CO2) is a disinfectant used in municipal water treatment plants. It dissolves in basic solution producing ClO3 and CLO2: 2 ClO2(g) +2 OH(aq) → ClO3(aq) + ClO2 (aq) + H2O(l) The following kinetic data were obtained at 298 K for the reaction. Experiment [ClO2]0 (M) [OH]o (M) Initial Rate (M/s) 1 0.060 0.030 0.0248 2 0.020 0.030 0.00827 3 0.020 0.090 0.0247 Determine the rate law by indicating the values of "x" and "y" in the general rate law below. Rate = k[CO2]*[OH-] x= Select an answer✔ y = Select an answer b. Calculate the rate constant for this reaction at 298 K. Sig. Figs. are important. Rate constant, k = M-1 s-1
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