The following initial rate data are for the reaction of ammonium ion with nitrite ion in aqueous solution:NH4+ + NO₂-N2 + 2 H₂OExperiment [NH4+]o, M [NO₂ ]o, M1234Rate =0.2940.294Submit Answer0.5880.5888.88×10-20.1788.88×10-20.178From these data, the rate constant isInitial Rate, Ms-18.04x10-61.61x10-5Complete the rate law for this reaction in the box below.Use the form k[A]”[B]". If m or n are 1, don't enter the 1. Omit concentrations taken to the zero power.1.61x10-53.22x10-5M-¹S-1.Try Another Version 7 item attempts remaining

The following initial rate data are for the reaction of ammonium ion with nitrite ion in aqueous solution: NH4+ + NO₂™ →N2 + 2 H₂O Experiment [NH4+]o, M [NO₂"]o, M Initial Rate, Ms-1 1 2 3 4 Rate = 0.294 0.294 Submit Answer 0.588 0.588 8.88x10-2 0.178 8.88x10-2 0.178 From these data, the rate constant is 8.04x10-6 1.61x10-5 Complete the rate law for this reaction in the box below. Use the form k[A][B]". If m or n are 1, don't enter the 1. Omit concentrations taken to the zero power. 1.61x10-5 3.22x10-5 M-¹S-1. Try Another Version 7 item attempts remaining

The following initial rate data are for the reaction of ammonium ion with nitrite ion in aqueous solution: NH4+ + NO₂™ →N2 + 2 H₂O Experiment [NH4+]o, M [NO₂"]o, M Initial Rate, Ms-1 1 2 3 4 Rate = 0.294 0.294 Submit Answer 0.588 0.588 8.88x10-2 0.178 8.88x10-2 0.178 From these data, the rate constant is 8.04x10-6 1.61x10-5 Complete the rate law for this reaction in the box below. Use the form k[A][B]". If m or n are 1, don't enter the 1. Omit concentrations taken to the zero power. 1.61x10-5 3.22x10-5 M-¹S-1. Try Another Version 7 item attempts 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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Question 4 Calculate the frequency factor (A). Studies have shown that the reaction occurs via the following mechanism. ki Cl2O4 k-1 Step 1: 2 Cl02 (fast equilibrium) k2 Step 2: C2O4 + OH- → ClO;¯+HCIO2 (slow) k3 Step 3: HCIO2 + OH → ClO2¯+H2O (fast) Question 5: Identify the intermediate/s and the rate-determining step. ki 2 ClO2 2 C2O4 k-1 Step 1: (fast equilibrium) k2 → ClO3¯+HC1O2 Step 2: C204 + OH- (slow) k3 Step 3: HC1O2 + OH- ClO2- + H2O (fast) Question 6 Is the proposed mechanism consistent with the experimentally determined rate law? Show your solution to justify your answer. ki 2 ClO2 2 C2O4 k-1 Step 1: (fast equilibrium) k2 Step 2: C204 + OH- → ClO3¯+ HCIO2 (slow) k3 Step 3: HCIO2 + OH- → ClO2-+ H2O (fast) Question 7 Draw the transition state for Step 3. Identify the bond/s forming/breaking.
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4. The following data were obtained for the follwing chemical reaction: 2A + 3B ---> 2C + D Initial [A] Initial [B] Initial Rate of Formation Trial # (mmol/L) (mmol/L) of D (mmol/L*s) 1 4.0 6.0 1.60 2 2.0 6.0 0.80 3 4.0 3.0 0.40 (a) Determine the rate law equation for this reaction. Show your reasoning. (b) Find the rate constant, k, with units.
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2. Consider the reaction A+2B C whose rate at 25 °C was measured using three different sets of initial concentrations as listed in the following table: [v] (M) (M) (M/s) [B] Rate Trial 1 0.10 0.050 6.0x10-4 0.10 0.100 1.2x10-3 3 0.20 0.050 2.4x10-3 Part B Provide
A Moving to another question will save this response. Question 24 The rate law for the reaction below is rate = k[N21*[H2]Y 2 NH3 N2 + 3 H2 - Which of the following is true? OA.x = 3 and y = 1 OB. The reaction is 4tn order overall OC The order of reaction needs to be determined experimentally O D.X = 1 and y = 1 OE.x = 1 and y = 3 A Moving to another question will save this response. MacBook esc F1 F2 F4 FS 23 3 4. tab aps lock F
Use this data to determine the value of the rate constant. Ex # [A] (M) [B] (M) Rate (M/hr) 1 .240 .120 2.00 2 .120 .120 .500 3 .240 .0600 1.00 Question 4 options: 289 per hour 579 per hour 8.3 per hour 0.0144 per hour 69.4 per hour .00346 per hour 0.060 per hour 0.0173 per hour 17 per hour 0.12 per hour
Consider the following complex reaction: A + 2B → C whose initial rate at 25 °C was measured using three different sets of initial concentrations as listed in the following table: Trial [A](M) [B](M) Rate(M/s) 1 0.400 0.050 9.60 × 10−3 2 0.400 0.100 1.92 × 10−2 3 0.800 0.050 3.84 × 10−2 A) Write the rate law for this reaction. Use k to represent the rate constant. B) Solve for k in the above rate law. Express your answer to three significant figures. Include units for k.
Use the previous example for the chemical reaction 2 HgCl₂(aq) + C₂O4²-(aq)→ 2 Cl(aq) + 2 CO₂ (g) + Hg₂Cl₂ (s) The following initial rates of reactions were determined for the reactant concentrations given: Experiment #[HgCl₂] 0.100 0.100 0.050 1 2 3 [C₂O4²-] 0.20 0.40 1.2 x 10-4 0.40 6.2 x 10-5 Initial rate (M/sec) 3.1 x 10-5 (a) Find the order of the reaction with respect to HgCl2₂. (b)Find the order of the reaction with respect to C₂04² (c)Write the rate law for this reaction. (d)Calculate the value for the rate constant based on the data for experiment #1 and provide the proper units.
Values if needed for this question. The following initial rate data are for the reaction of mercury(II) chloride with oxalate ion: 2 HgCl2 + 2 CI + Hg,Cl2 + 2 CO2 Experiment [HgCl2]o, M [C,0,?], M Initial Rate, M sl 1 0.415 0.180 1.23x104 0.830 0.180 2.45x104 4.91×10-4 9.81×104 3 0.415 0.360 4 0.830 0.360 Complete the rate law for this reaction in the box below. Use the form k[A]™[B]" , where '1' is understood for m or n and concentrations taken to the power not appear. Don't enter 1 for m or n. Rate = From these data, the rate constant is M2s1 Submit Answer Try Another Version 2 item attempts remaining
How would you find the rate law for this question?
Consider the following complex reaction: 2NO2(g) + O3(g) → N2O5(g) + O2(g) whose initial rate at 25 °C was measured using three different sets of initial concentrations as listed in the following table: Trial [NO2](M) [O3] (M) Rate (M/s) 1 0.20 0.40 0.25 2 0.40 0.40 0.50 3 0.40 1.20 1.50 What is the rate law for this reaction? Write the value for k to two significant figures in the first box. Select the units for k and concentration terms in the second box.