1. Consider these three reactions as the elementary steps in the mechanism for a chemical reaction. (i) H2(g) + NO(g) → H20(g) + N(g) (ii) N(g) + NO(g) → N2(g) + O(g) (iii) O(g) + H2(g)→ H20(g) Ea = 436 kJ AH = -491 kJ Ea = 625 kJ AH = -312 kJ Ea = 1690 kJ AH = +131 kJ a. What is the AH for the overall reaction? Overall, is it endothermic or exothermic? b. Draw the potential energy diagram for the reaction. Assume the potential energy of the reactants was 1400 kJ 2600 2400 2200 2000 1800 1600 1400 1200 1000 800 600 400 200 Reaction Progress c. What is E, for the overall reaction? You must calculate this from the potential energy diagram. Potential Energy (kJ)

1. Consider these three reactions as the elementary steps in the mechanism for a chemical reaction. (i) H2(g) + NO(g) → H20(g) + N(g) (ii) N(g) + NO(g) → N2(g) + O(g) (iii) O(g) + H2(g)→ H20(g) Ea = 436 kJ AH = -491 kJ Ea = 625 kJ AH = -312 kJ Ea = 1690 kJ AH = +131 kJ a. What is the AH for the overall reaction? Overall, is it endothermic or exothermic? b. Draw the potential energy diagram for the reaction. Assume the potential energy of the reactants was 1400 kJ 2600 2400 2200 2000 1800 1600 1400 1200 1000 800 600 400 200 Reaction Progress c. What is E, for the overall reaction? You must calculate this from the potential energy diagram. Potential Energy (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...

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At 20°C the rate of a reaction 2 H₂O₂ à 2 H₂O + O₂ is 3.0 x 10¹ M/s. What is a good estimate for the rate of this reaction at 30°C? O 9.0 x 10-2 M/s O 1.5 x 101 M/s 3.0 x 101 M/s O 5.5 x 101 M/s 6.0 x 10¹ M/s
Consider these three reactions as the elementary steps in the mechanism for a chemical reaction. (i) H2(g) + NO(g) à H2O(g) + N(g) Ea = 436 kJ ∆H = –491 kJ (ii) N(g) + NO(g) à N2(g) + O(g) Ea = 625 kJ ∆H = –312 kJ (iii) O(g) + H2(g) à H2O(g) Ea = 1690 kJ ∆H = +131 kJ Draw the potential energy diagram for the reaction. Assume the potential energy of the reactants was 1400 kJ
Consider these three reactions as the elementary steps in the mechanism for a chemical reaction. (i) H2(g) + NO(g) à H2O(g) + N(g) Ea = 436 kJ ∆H = –491 kJ (ii) N(g) + NO(g) à N2(g) + O(g) Ea = 625 kJ ∆H = –312 kJ ( iii) O(g) + H2(g) à H2O(g) Ea = 1690 kJ ∆H = +131 kJ What is the ∆H for the overall reaction? Overall, is it endothermic or exothermic?
When the energy of activation is low, many molecules have enough energy to cross the energy barrier and the reaction is fast. A) True False Gp 么 -> esc # $4 ! 7 1 2 3 4 e r t tab d f j a 00 く
O 11. The decomposition of ozone in the upper atmosphere to dioxygen occurs by a two-step mechanism. The first step is a fast reversible step and the second is a slow reaction between an oxygen atom and an ozone molecule: Step 1: Step 2: O3(g) = 02(8) + O(g) O3(g) + 0(g) → 202(g) Fast, reversible, reaction Slow a. Which is the rate determining step? b. Write the rate equation for the rate-determining step. Write the rate equation for the overall reaction. с. The rate equation for the reaction of nitrogen dioxide and carbon monoxide in the gas state to form carbon dioxide and nitric oxide is represented by the equation: 12. NO2(g) + CO(g) → NO(g) + CO2(g) The following data were collected at 125°C:e Experiment 1 Experiment 2 Experiment 3 Initial [NO2] mol L 5.0 x 104 5.0 x 104 1.5 x 10-3 Initial [CO] mol L- 1.6 x 10-2 3.2 x 102 3.2 x 10-2 Initial rate mol L'min 1.7 x 10-7 1.7 x 10-7 1.5 x 10-6 What is the order with respect to NO2? b. What is the order with respect to CO? c. What is the…
13. A reaction A+B+C → D follows the mechanismA  B   C A B  C   Din which the first step remains essentially in equilibrium. Show that the dependence of rate on temperature is given byk  Ae(Ea H )/RTwhere H is the enthalpy change for the first reaction.
Derive the unit for K then using K at 904 degrees celsius, find the rate of reaction at the instant when [NO]=0.470 M and [H2] = 0.315M
Consider the reaction 2 D(g) + 3 E(g) + F(g) → 2 G(g) + H(g). When [E] is decreasing at 0.10 mol/ L-s, how fast is [D] decreasing? (Disregard the use of any negative sign.) 0.30 mol/ L-s 0.15 mol/ L-s None of these 0.10 mol/ L-s 0.067 mol/ Ls
Which of the following reactions is impossible to occur as a single step? Cl2(g) --> 2 CI(g) OCI + H20(1) --> HOCI(aq) + OH NO(g) + Cl2(g) NOCI2(g) --> O 2 NO(g) + O2(g) 2 NO2(g) -->
Potentially Useful Reference Information -Ea J R = 8.314 k = A· e RT mol ·K Complete the sentences below regarding the following reaction: CH4 + 2 O2 → CO2 + 2 H2O Methane (CH4) as water (H2O) The rate that oxygen (O2) is as the rate carbon dioxide (CO2) The possible answers are: appears, disappears, half as fast, twice as fast, or at the same rate.