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

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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

Initial-rate data at a certain temperature is given in the table for the reaction SO₂Cl₂(g) → SO₂(g) + Cl₂(g) [SO₂Cl₂], (M) k= 0.100 0.200 0.300 Initial rate (M/s) 1.90 x 10-6 3.80 x 10-6 5.70 x 10-6 Determine the value and units of the rate constant. units:

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

Derive the unit for K then using K at 904 degrees celsius, find the rate of reaction at the instant when [NO]=0.470 M and [H2] = 0.315M

Use this data for the following four (4) questions: The relative initial rates of the reaction A2 + B2-products in vessels (a)-(d) are 1:1:4:4. The spheres represent the number of molecules of present at the beginning of the reaction. [Unshaded spheres = A2 molecules; shaded spheres = B2 molecules] %3D For example, vessel (a) contains 2 A2 molecules and 2 B2 at the beginning of the reaction. Rate = 1 Rate 1 Rate = 4 Rate = 4 %3D 2. 8. 80 (c) (a) 11) What is the order of reaction with respect to A2? (b) (d) BA 11) A))0 B) 1 C) 2 D) 3 12) What is the order of reaction with respect to B2? 12) C A) 0 B) 1 D) 3 13) o c 13) What is the overall order of reaction? A) 0 B) 1 D) B 14) 14) What is the rate law for this reaction? B) Rate k[B2]2 D) Rate = k[A2]2[B2]² A) Rate = k[A2]² %3D C) Rate = k[A2][B2] %3D %3D nation below: 15) 8. 8.