Suppose the formation of dinitrogen pentoxide proceeds by the following mechanism: step elementary reaction 1 NO₂ (g) +03 (g) → NO3 (g) + O₂ (g)| 2 NO3 (g) + NO₂ (g) → N₂O5 (8) Suppose also k₁ « k₂. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction. Write the experimentally- observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates. 0 rate = k rate constant k₁ k₂

Suppose the formation of dinitrogen pentoxide proceeds by the following mechanism: step elementary reaction 1 NO₂ (g) +03 (g) → NO3 (g) + O₂ (g)| 2 NO3 (g) + NO₂ (g) → N₂O5 (8) Suppose also k₁ « k₂. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction. Write the experimentally- observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates. 0 rate = k rate constant k₁ k₂

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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The reaction O₂(g) + 2 NO(g) → 2 NO₂(g) was studied at a certain temperature with the following results: (a) What is the rate law for this reaction? O Ratek [0₂(9)] [NO(g)] O Ratek [0₂(9)]² [NO(g)] O Rate = k [0₂(9)] [NO(g)]² O Ratek [0₂(9)]² [NO(g)]² O Ratek [0₂(9)] [NO(g)]³ O Rate = k [O₂(g)]* [NO(g)] (b) What is the value of the rate constant? Experiment [0₂(9)] (M) 0.0235 0.0235 0.0470 0.0470 [NO(g)] (M) 0.0235 0.0470 0.0235 0.0470 Rate (M/S) 0.158 0.633 0.317 1.27 (c) What is the reaction rate when the concentration of O₂(g) is 0.0318 M and that of NO(g) is 0.0649 M if the temperature is the same as that used to obtain the data shown above?
Organic compounds that contain large proportions of nitrogen and oxygen tend to be unstable and are easily decomposed. Hexanitroethane, C2(NO2)6, decomposes according to the equation C2(NO2)6- 2NO2 + 4NO + 2CO, The reaction in CCI, solvent is first order with respect to C2(NO2)6. At 78.9°C, k = 0.000303 s1 and at 107.4 °C, k = 0.0207 s1. (a) What is the half-life of C2(NO2)6 at 78.9°C? i seconds eTextbook and Media (b) What is the half-life of C2(NO2)6 at 107.4 °C? i seconds (c) If 0.100 mol of C2(NO2)6 is dissolved in CCI4 at 78.9°C to give 1.00 L of solution, what will be the C2(NO2)6 concentration after 50.0 minutes? i M (d) What is the value of the activation energy of this reaction, expressed in kilojoules? i kJ/mol
Consider the reaction 2NO(g) + O2(g) → 2NO2(g) Suppose that at a particular moment during the reaction nitric oxide (NO) is reacting at the rate of 0.066 M/s. (a) At what rate is NO2 being formed? (b) At what rate is molecular oxygen reacting?
The balanced chemical equation for the reaction between iodine vapour and fluorine gas is: 3I2(g) + 6F2(g) → 2IF5(g) + I 4F 2(g) A chemist measures the rate at which iodine vapour is consumed to be 4.5 × 10–4 mol/(L•s). At what rate is F2(g) consumed?
Enter your answer in the provided box. Consider the reaction: N2(g) + 3H2(g) → 2NH3(g) Suppose that a particular moment during the reaction, molecular hydrogen is reacting with a magnitude of 0.0227 M/s. At what rate is molecular nitrogen reacting?
Suppose the reduction of nitric oxide proceeds by the following mechanism: step elementary reaction rate constant 1 H, (g) + 2NO (g) → N,0 (g)+ H,0 (g) k1 H, (g) + N,0 (g) → N2 (g) + H20 (g) k2 Suppose also k, « k,. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction. Write the experimentally- observable rate law for the overall chemical reaction. rate = k|| Note: your answer should not contain the concentrations of any intermediates.
The rate constant for the reaction 2N2O5(g) → 4NO2(g) + O2(g) is equal to 3.41 x 10–5 s–1 at 30 ºC. If the initial concentration of N2O5is 0.446 M what concentration of NO2 will be observed after 175 minutes? Assume that initially no NO2 was present in the reaction vessel.
The reaction between nitric oxide and bromine is described by the following chemical equation: 2NO (g) + Br, (g) – 2NOB (g) Suppose a two-step mechanism is proposed for this reaction, beginning with this elementary reaction: NO (g) + Br, (g) NOB12 (g) Suppose also that the second step of the mechanism should be bimolecular. Suggest a reasonable second step. That is, write the balanced chemical equation of a bimolecular elementary reaction that would complete the proposed mechanism.
Suppose the formation of iodine proceeds by the following mechanism: step elementary reaction 1 H₂(g) + IC1 (g) → HI(g) + HC1 (g) k₁ 2 HI (g) + IC1 (g) → I₂ (g) + HCl (g) k₂ Suppose also k₁ « k₂. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction. Write the experimentally- observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates. 0 rate = k rate constant
A reaction proceeds according to the following equation: A + 3B → 2C + 2D At an early stage of the reaction, conc. A = 1.191 M and 6.06 minutes later, conc. A= 0.949 M. What is the average rate of the reaction during this time period, expressed in units of M·s-1?
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
Consider the reaction : 3A + 2B → 4C Initially, and at some fixed temperature, the reaction proceeds at such a rate that 2.3 millimoles of A are consumed in 1 minute and 12 secondes. The reaction takes place in 1 L. The following table contains the experimental data for the reaction. (Taken from Ball. Physical Chemistry, 2nd edition, 2006) Rate (M/s) [A], M [B], M 1.081 x 10-5 0.660 1.23 6.577 x 10-5 4.01 1.23 6.568 x 10-5 4.01 2.25 c. Determine the partial order on A. Partial order on B is 0. d. What is the order of the reaction.