a. Given the balanced equation: C,H,(g) + 50₂(g) 3CO₂(g) + 4H₂O(g) and the data below,calculate the average rate of propane (C₂Hg) between 20.0 and 50.0 seconds.Time, sC3H8], MD.A0.00.26- (ма-матtf-ti10.00.1820.00.14-30.00.10Write the rate expression for this reaction. [₁]-^ [C3H8] +-=A[02]ALLOT+4D +307SA+At.50.000.052- (₁052 -0.14) M- .00 29/(50.0 -20.0)840.00.064Use the information in part a to calculate the rate of CO₂ in this same time period.A [10₂].0087 M/S3mol CO₂--0029cs Hars. Imol C3H8 d.What is the rate of this reaction between 20.0 and 50.0 sec

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Answered: a. Given the balanced equation: C,H,(g)…

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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4. The following data were obtained for the follwing chemical reaction: 2A+38->2C+D Trial # Initial (A) Initial [B] Initial Rate of Formation (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. (T: 2) (b) Find the rate constant, k, with units. (T: 2)
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A + B → C [A](M)[B](M) Initial Rate (M/h) 0.137 0.277 193 0.428 0.277 1,470 0.137 0.679 547 Find the order with respect to B. Round to the nearest whole number.
The reaction 2 N205(g) → 4 NO2(g) + O2(g) was studied and the rate of change of the concentration of O2 was found to be 3.65 mol L 15-1. Calculate the reaction rate (in mol L1s1). Reaction rate = i mol L-1s-1. eTextbook and Media Save for Later Attempts: 0 of 3 used Submit Answer
2NO(g) +O2(g) → 2NO(g) The following kinetic data were obtained for the initial rates of disappearance of NO: Expriment Initial Conc. of NO Initial Conc. of O2 Initial Rate Exp. 1 0.0125 M 0.0253 M 0.0281 M/s Exp. 2 0.0250 M 0.0253 M 0.112 M/s Exp. 3 0.0125 M 0.0506 M 0.0561 M/s What is the value of the rate constant for the reaction? Express your answer to three significant figures. Just enter the number (e.g. 2.48x10^-4) and the unit.
For the hypothetical reaction A + 2B 3C, the rate of appearance of C given by (A[C]/At) may also be expressed as O A[C]/At = -(2/3) A[B]/At O A[C]/At = -(3/2) A[B]/At O A[C]/At = -(1/2) A[A]/At %3D O A[C]/At = A[A]/At
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Nitrogen monoxide reacts with oxygen to give nitrogen dioxide. 2NO(9) + 02 (9) → 2NO: (9) The rate law is A[NO] At - k[NO]°[02] where the rate constant is 1.16 x 10-5 L/(mol? . s) at 339°C. A vessel contains NO and Oz at 339°C. The initial partial pressures of NO and Oz are 157 mmHg and 348 mmHg, respectively. What is the rate of decrease of partial pressure of NO? (Hint: From the ideal gas law, obtain an expression for the molar concentration of a particular gas in terms of its partial pressure.) Rate =
Be sure to answer all parts. For the following general reaction, rate = k[A]2 and k=1.3 × 10 2 M¹g¹; A+B 2C Use this information to fill in the missing table entries. Experiment [A] (M) [B] (M) Initial rate (M/s) 1 0.013 0.250 2.20 × 10-6 2 0.026 0.250 3 0.500 2.20 × 10-6 1) Initial reaction rate in experiment 2: x 10 M/s (Enter your answer in scientific notation.) 2) Initial concentration of A in experiment 3: M
The rate of decomposition of A into B and C at 25 °C is found to be 1.35 x 10-4 M A/min. What is the rate at which C is produced? 2 A (aq) > 3 В (аq) + C (аq) Select one: а. 2.03 х 10-5М (/min b. 1.35 x 10-4 M C/min -5 с. 9.00 х 10 М C/min d. 2.70 x 10-4 M C/min e. 6.75 х 10-5М (/min
Part A Consider the balanced chemical equation. H2O2(aq) + 3I¯ (aq) + 2H+(aq) → I3 (aq) + 2H20(1) Predict the rate of change in the concentration of H2O2 (A[H2O2]/At). In the first 12.0 s of the reaction, the concentration of I drops from 1.000 M to 0.773 M . Express the rate to three significant figures and include the appropriate units. You may want to reference (Pages 587 - 592) Section 14.3 while completing this problem. ? A[H2O2]/At = Value Units
Given the following reaction, 2 NH3(g) → N2(g) + 3 H2(g) Which of the following relates the appearance of H2 to the disappearance of NH3? A) rate of appearance H2 = 3/2 ( △NH3 / △t ) B) rate of appearance H2 = 1/2 ( △NH3 / △t ) C) rate of appearance H2 = - 2/3 ( △NH3 / △t ) D) rate of appearance H2 = - 3/2 ( △NH3 / △t ) E) rate of appearance H2 = - 1/2 ( △NH3 / △t )

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