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3. Consider the reaction shown below and the tabulated experimental data on initial rates. A +B + 2 C →D+E Table 1. Initial concentrations of reactants and the corresponding rates at 25 °C Rate (M/s) [A]; (M) [B]; (M) [C]; (M) 0.390 0.10 0.10 0.30 0.130 0.10 0.10 0.10 0.975 0.10 0.25 0.30 0.585 0.15 0.10 0.30 A. Determine the reaction order with respect to A, B, and C. B. Calculate the average rate constant for the reaction. C. What is the rate law for the reaction and the overall reaction order? D. Calculate the activation energy (Ea) for the reaction assuming that the frequency factor (A) is 1.23 x 1010 /M's. E. What is the rate constant at 50 °C?

3. Consider the reaction shown below and the tabulated experimental data on initial rates. A +B + 2 C →D+E Table 1. Initial concentrations of reactants and the corresponding rates at 25 °C Rate (M/s) [A]; (M) [B]; (M) [C]; (M) 0.390 0.10 0.10 0.30 0.130 0.10 0.10 0.10 0.975 0.10 0.25 0.30 0.585 0.15 0.10 0.30 A. Determine the reaction order with respect to A, B, and C. B. Calculate the average rate constant for the reaction. C. What is the rate law for the reaction and the overall reaction order? D. Calculate the activation energy (Ea) for the reaction assuming that the frequency factor (A) is 1.23 x 1010 /M's. E. What is the rate constant at 50 °C?

Chemistry
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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2. Consider the following reaction and the tabulated thermochemical data at 298 K. 4 NH3(2) + 5 O2(g) → 6 H2O(g) + 4 NO(2) Substance NH3(g) Ozg) H2O(g) NO(2) AH°r (kJ/mol) -46.1 -241.8 90.3 S° (J/mol-K) 192.3 205.0 188.7 210.7 A. Calculate the standard enthalpy change of the reaction in kJ. Is the process endothermic or exothermic? B. Calculate the standard entropy change of the reaction in J/K. C. Calculate the standard Gibbs free energy change of the reaction in kJ at 298 K. Is the reaction spontaneous at 298 K? D. Calculate the equilibrium constant at 298 K. E. Calculate the Gibbs free energy change at 298 K for a mixture containing 2.0 atm NH3(g), 1.0 atm Oz(g), 1.5 atm H2O(g), and 1.2 atm NO(g). 3. Consider the reaction shown below and the tabulated experimental data on initial rates. A+B + 2 C →D+E Table 1. Initial concentrations of reactants and the corresponding rates at 25 °C Rate (M/s) [A]; (M) [B]; (M) [C]; (M) 0.390 0.10 0.10 0.30 0.130 0.10 0.10 0.10 0.975 0.10 0.25 0.30 0.585 0.15 0.10 0.30 A. Determine the reaction order with respect to A, B, and C. B. Calculate the average rate constant for the reaction. C. What is the rate law for the reaction and the overall reaction order? D. Calculate the activation energy (Ea) for the reaction assuming that the frequency factor (A) is 1.23 x 1010 /M?s. E. What is the rate constant at 50 °C?
Transcribed Image Text:2. Consider the following reaction and the tabulated thermochemical data at 298 K. 4 NH3(2) + 5 O2(g) → 6 H2O(g) + 4 NO(2) Substance NH3(g) Ozg) H2O(g) NO(2) AH°r (kJ/mol) -46.1 -241.8 90.3 S° (J/mol-K) 192.3 205.0 188.7 210.7 A. Calculate the standard enthalpy change of the reaction in kJ. Is the process endothermic or exothermic? B. Calculate the standard entropy change of the reaction in J/K. C. Calculate the standard Gibbs free energy change of the reaction in kJ at 298 K. Is the reaction spontaneous at 298 K? D. Calculate the equilibrium constant at 298 K. E. Calculate the Gibbs free energy change at 298 K for a mixture containing 2.0 atm NH3(g), 1.0 atm Oz(g), 1.5 atm H2O(g), and 1.2 atm NO(g). 3. Consider the reaction shown below and the tabulated experimental data on initial rates. A+B + 2 C →D+E Table 1. Initial concentrations of reactants and the corresponding rates at 25 °C Rate (M/s) [A]; (M) [B]; (M) [C]; (M) 0.390 0.10 0.10 0.30 0.130 0.10 0.10 0.10 0.975 0.10 0.25 0.30 0.585 0.15 0.10 0.30 A. Determine the reaction order with respect to A, B, and C. B. Calculate the average rate constant for the reaction. C. What is the rate law for the reaction and the overall reaction order? D. Calculate the activation energy (Ea) for the reaction assuming that the frequency factor (A) is 1.23 x 1010 /M?s. E. What is the rate constant at 50 °C?
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