1. Given the experimental data below, ⚫ determine the rate law equation, • Total Order of the reaction and ⚫ the rate constant, k, for the following reaction. • 3A (aq) + 2B (aq) --> products Reaction Rate (mol L-1 s [A] mol/L [B] mol/L 1) 1 0.400 0.100 1.50 x 10-3 2 1.600 0.100 1.50 x 10-3 3 0.400 0.500 3.75 x 10-2 The combustion of methanol is shown by the following equation: 2CH3OH (1) + 302(g) >2CO2(g) + H2O (8) Given the data which follows: a. Find the enthalpy of reaction for the equation above. b. State whether the reaction is endothermic or exothermic. C(s) + O2(g) 2(g) + 393 kJ H2(g) + 0₂ 2(g) >H₂O(g) +242 kJ C(s) + 2H2(g) + O2(g) -> CH₂OH (n) + 638 kJ

1. Given the experimental data below, ⚫ determine the rate law equation, • Total Order of the reaction and ⚫ the rate constant, k, for the following reaction. • 3A (aq) + 2B (aq) --> products Reaction Rate (mol L-1 s [A] mol/L [B] mol/L 1) 1 0.400 0.100 1.50 x 10-3 2 1.600 0.100 1.50 x 10-3 3 0.400 0.500 3.75 x 10-2 The combustion of methanol is shown by the following equation: 2CH3OH (1) + 302(g) >2CO2(g) + H2O (8) Given the data which follows: a. Find the enthalpy of reaction for the equation above. b. State whether the reaction is endothermic or exothermic. C(s) + O2(g) 2(g) + 393 kJ H2(g) + 0₂ 2(g) >H₂O(g) +242 kJ C(s) + 2H2(g) + O2(g) -> CH₂OH (n) + 638 kJ

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

kinetic data for the following reaction was determined experimentally; 2NO(g) + Chlg) - 2NOCI(g) Experiment number [Ch). M 0.20 [NO). Initial rate of reaction M 0.10 0.30 M/s 0.63 5.70 0.20 0.80 2 0.10 2.58 The orders of the reaction with respect to NO and Cly are respectively. and O two and one, respectively. O one and two, respectively. O three and one respectively. O one and three, respectively,
Payalben
Consider the following reaction: A + B --> products. The rate law was found to be rate = k[A][B]^2. If the concentration of B is doubled while the concentration of A is halved, how will this affect the rate of the equation? How will this affect the time required for the reaction to reach completion?
From the data given in the table below, determine the rate law for the following chemical equation. NH4+(aq) + NO2-(aq) → N2(g) + 2 H2O(l) Experiment [NH4+]o [NO2-]o Initial Rate (consumption of NH4+) 1 0.24 0.10 7.2 x 10-6 M/s 2 0.12 0.10 3.6 x 10-6 M/s 3 0.12 0.15 5.4 x 10-6 M/s Select one: a. Rate = k[NH4+][NO2-]2 b. Rate = k[NH4+]2[NO2-] c. Rate = k[NH4+]2 d. Rate =k[NH4+]2[NO2-]2 e. Rate = k[NO2-] f. Rate = k[NO2-]2 g. Rate = k[NH4+] h. Rate = k[NH4+][NO2-]
The balanced equation for a given reaction is 4 X + 3 Y → P. The following data regarding initial reaction rates were collected in the lab. What is the rate law for the reaction? Trial [X] (M) [Y] (M) Rate (M/s) 1 0.020 0.060 3.40 x 10–3 2 0.020 0.120 2.72 x 10–2 3 0.080 0.060 1.36 x 10–2
Using the data in the table, calculate the rate constant of this reaction. k= A+B → C + D Trial [A] (M) [B] (M) 1 0.290 0.380 2 0.290 1.03 3 0.464 0.380 Units Rate (M/s) 0.0163 0.119 0.0261
Initial rates were measured for the following reaction and are listed in the table. A + 2B ⎯→ products Expt. Initial Concentrations Initial Rate (mol/L·s) [A] [B] 1 0.115 0.135 2.70 × 10−3 2 0.115 0.270 2.16 × 10−2 3 0.345 0.135 8.10 × 10−3 What is the order of the reaction with respect to A, with respect to B, and overall?
The rate of a certain reaction is given by the following rate law: rate=k H2 | I2| *[H:]L] Use this information to answer the questions below. What is the reaction order in H,? What is the reaction order in I,? ? What is overall reaction order? At a certain concentration of H2 and I2, the initial rate of reaction is 34.0 M / s. What would the initial rate of the reaction be if the concentration of H2 were halved? Round M S your answer to 3 significant digits. The rate of the reaction is measured to be 0.530 M/ s when [H2] = 1.4 M and [I2] = 0.21 M. Calculate the value of the - 1 - 1 k = |M •S rate constant. Round your answer to 2 significant digits.
Some measurements of the initial rate of a certain reaction are given in the table below. [N-] N2 H2 initial rate of reaction 1.27M 0.589М 22.0M/s 1.27 M |0.149 М 5.57 M/s 0.445 M 0.589M 2.70M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol. rate = k |I| х10 k =
Consider the reaction I- + OCl- → OH-→ IO- + Cl- Determine the reaction's rate law using the given experimental data. Exp # [I-]o [OCl-]o [OH-]o Initial Rate (M/s) 1 0.0013 0.012 0.10 0.094 2 0.0026 0.012 0.10 0.187 3 0.0013 0.006 0.10 0.047 4 0.0013 0.012 0.20 0.047
Some measurements of the initial rate of a certain reaction are given in the table below. [N-] H2 initial rate of reaction 4 0.756M 0.169M 5.00 x 10*M/s 0.186M 0.169M 3.03 × 10°M/s olo 0.756M 0.0761 M 2.25 x 10*M/s Ar Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol. rate = k [] Ox10 k = 0