For the reaction CgHg + 502 + 3 CO2 + 4H2O which of the following is a valid expression for the reaction rate? (A) Δ[C3Hg] Δt (B) –5 41021 (Β) (C) - - 1 Δ[02] Δt (Ε) 3 5 (D) —4 4[H,0] Δt Δ[CO2] Δ

For the reaction CgHg + 502 + 3 CO2 + 4H2O which of the following is a valid expression for the reaction rate? (A) Δ[C3Hg] Δt (B) –5 41021 (Β) (C) - - 1 Δ[02] Δt (Ε) 3 5 (D) —4 4[H,0] Δt Δ[CO2] Δ

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...

See similar textbooks

Similar questions

Be sure to answer all parts. Acetone is one of the most important solvents in organic chemistry. It is used to dissolve everything from fats and waxes to airplane glue and nail polish. At high temperatures, it decomposes in a first- order process to methane and ketene (CH,=C=0). At 600°C, the rate constant is 8.7 x 103 s1. (a) What is the half-life of the reaction? Give your answer in scientific notation. x 10 (select) A (b) How long does it take for 42% of a sample of acetone to decompose? (c) How long does it take for 82% of a sample of acetone to decompose? Give your answer in scientific notation. x 10 (select) O S
4. Given the following data for this reaction: The rate law for the reaction is: (a) Rate = k[NH4"][NO₂] (b) Rate = k[NH4']2[NO₂]² (c) Rate = k[NH4+]2[NO₂] (d) Rate = k[NH4+][NO₂1² (e) none of the above NH4+ (aq) + NO₂ (aq) → N₂(g) + 2H₂O(1) EXPT [NH4] [NO₂] RATE 1 2 3 0.010 M 0.015 M 0.010 M 0.020 M 0.020 M/s 0.020 M 0.030 M/s 0.010 M 0.005 M/s
Identify each of the following elementary reactions as uni- molecular, bimolecular, or termolecular, and write the rate expression. (a) HCO + O2 → HO2 + CO (b) CH3 + O2 + N2 → CH;O2 + N2 (c) HO,NO2 –→ HO2 + NO2
The decomposition of XY is second order in XY and has a rate constant of 7.41 × 10−3 L·mol−1·s−1 at a certain temperature, the half-life for this reaction at an initial concentration of 0.101 mol·L−1 1336. A) If the initial concentration of XY is 0.225 mol·L−1, how long will it take for the concentration to decrease to 6.95 × 10−2 mol·L−1 ?, B) If the initial concentration of XY is 0.080 mol·L−1, what is the concentration of XY after 75 s ?
The gas phase reaction of iodine with silane takes place according to a second-order reaction: I2(g) +SİH4(g)–→HI(g) +SIH3I(g) The activation energy is Ea = 83.2 kJ mol-1. At 269°C, the reaction rate constant is 3.49 L mols. (a) Calculate the Arrhenius factor A for this reaction. L mols1 (b) Calculate the rate constant for this reaction at 235°C. L molls1
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?
(4a) The following initial rate data are for the reduction of nitric oxide with hydrogen:2 NO + 2 H2N2 + 2 H2O Experiment [NO]o, M [H2]o, M Initial Rate, M s-1 1 0.438 0.289 7.93×10-2 2 0.876 0.289 0.317 3 0.438 0.578 0.159 4 0.876 0.578 0.634 Complete the rate law for this reaction in the box below. Use the form k[A]m[B]n , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = From these data, the rate constant is ____________ M-2s-1. (4b) 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 0.710 0.152 3.38×10-5 2 0.710 0.303 6.73×10-5 3 1.42 0.152 6.76×10-5 4 1.42 0.303 1.35×10-4 Complete the rate law for this reaction in the box below. Use the form k[A]m[B]n , where '1' is understood for m or n and concentrations taken to the zero power do not…
Suppose the parent reaction: A + 2B AB2 occurs by the following mechanism: Step 1 A + B AB slow Step 2 AB + B AB2 fast The rate law expression of the parent reaction is Rate = (a) k[A][B]2 (b) k[B] (c) k[A][B] (d) none of these
??
help w this question plz
Identify each of the following elementary reactions as unimolecular, bimolecular, or termolecular, and write the rate expression. (a) O + H₂S Reaction HO + HS (b) OH + NO2 + N₂ HNO3 + N2 (c) CH3CHO → CH3 + CHO Molecularity. ][ Rate expression rate = rate = rate =
17. If one defines the rate of the reaction 30 CH3OH +B10H14 0 10 B(OCH3)3 + 22 H2 as -A[B10 H14] At Rate = then the rate is also correctly expressed by 1 A[CH3 OH] At 1 ΔΒ(0CH> )s] At 1 A[H;] (a) Rate = 30 (b) Rate = 10 (c) Rate = 22 At (d) none of these. (e) all of these.