The activation energy for the reaction NO2(g) + CO(g) NO(g) + CO2 (g) is E = 100 kJ/mol and the change in enthalpy for the reaction is AH = -325 kJ/mol. What is the activation energy for the reverse reaction? Express your answer with the appropriate units. > View Available Hint(s) Ti HA Value Units

The activation energy for the reaction NO2(g) + CO(g) NO(g) + CO2 (g) is E = 100 kJ/mol and the change in enthalpy for the reaction is AH = -325 kJ/mol. What is the activation energy for the reverse reaction? Express your answer with the appropriate units. > View Available Hint(s) Ti HA Value Units

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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1:37 Search 1 4 The activation energy Ea for a particular reaction is 42.2 kJ/mol. How much faster is the reaction at 343 K than at 323 K? (R = 8.314 J/mol K) ● 7 2 +/- LO 5 Question 1 of 18 8 30 9 0 Tap here or pull up for additional resources 3 6 5G+ 68 Submit X с x 100
Reaction CaCO3(s) Ca²+ (aq) + CO3²- (aq) AgCl(s) Ag+ (aq) + Cl(aq) AgBr(s) = Ag*(aq) + Br(aq) Agl(s) Ag+ (aq) + I¯(aq) Initial Concentrations ← [Ca²+] = 1.0 x 10-⁹ M [CO32] = 1.0 x 10⁹ M Ksp = [Ca²+][CO3²-1 X = 3.8 x 10-9 Initial Conditions Q = [1.0 × 10-⁹][1.0 × 10-⁹] = 1.0 x 10-18 Equilibrium Conditions [Ca2+] = 1.0 x 10⁹ M [CO32] 1.0 x 10.⁹ M Mass of CaCO3(s) = 0.0 g 42 of 7 What is the value of the reaction quotient, Q, which is calculated by substituting the actual initial values of [Ca²+] and [CO32] into the equilibrium expression?
Energy (kJ)) 4. Consider the figure shown below in answering the questions: 160 140 120 100 80 60 40 20 0 T ▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬▬ Progress of reaction a) What is the energy of activation, Ea for the reaction? b) What is the AE for the reaction? c) Is the reaction exothermic or endothermic? kJ kJ
Consider the quilibrium reaction between X and Y, as shown below: X=Y AG The reaction is started with 10 mmol of X; no Y is initially present. After 48 hours, analysis reveals the presence of 10 mmol of X and 0 mmol of Y. Which is the most likely explanation? = −1 - 45 kJ mol X and Y have reached equilibrium concentrations. An enzyme has shifted the equilibrium toward X. Formation of Y is kinetically slow; equilibrium has not been reached by 48 hours. Formation of Y is thermodynamically unfavorable. Two of the above explanations are reasonable.
1. Which of the following conditions describe the two step reaction energy profile below? (choose all that apply) Ea PE - ΔΕ Reaction Coordinate The first step is the rate determining step The first step is exothermic The second step is the rate determining step The second step is exothermic The overall reaction is endothermic
The reaction for the decomposition of ammonia into its elements is: 2 NH3 (g) → N2 (g) + 3 H2 (g) [N2] 0.0105 M If the concentrations at a certain time are: what will be the associated value of the reaction quotient (Q)? [NH3] = 0.505 M [H2] = 0.414 M, %3D %3D (A) (B) (C) (D) (E) 0.00148 0.00292 0.00861 0.0105 342
The following reaction was studied in the laboratory and the data shown in the table below was recorded at 25oC : A(g) + B(g)⟶C(g) + D(g) Trial A (mol/L) B (mol/L) Δ[C]/Δt (mol/L/s) 1 1.00 × 10−6 3.00 × 10−6 6.60 × 10−5 2 1.00 × 10−6 6.00 × 10−6 1.32 × 10−4 3 1.00 × 10−6 9.00 × 10−6 1.98 × 10−4 4 2.00 × 10−6 9.00 × 10−6 3.96 × 10−4 5 3.00 × 10−6 9.00 × 10−6 5.94 × 10−4 (a) Determine the order of reaction with respect to each reactant and the overall order. Show your working clearly. (b) Determine the value of the rate constant K. (c) Calculate the half-life of the reactant ‘A’ if initial concentration is 1 x 10-6 M. (d) Using this reaction as an example, explain the difference between stoichiometric coefficients, reaction order and molecularity.
12:27 12-2 Analyzing Data... NAME Energy (kJ) NAME 1000 Many chemical reactions involve a change in energy. When the energy of the reactants is greater than the energy of the products, the reaction gives off heat and is exothermic. When the energy of the products is greater than that of the reactants, the reaction must absorb energy from the surroundings to occur and is endothermic. If the intermediate stage (the activated complex) is of a higher energy, then the reaction can only take place if the reactants are given an initial energy input (the activation energy). The graph shows energy diagrams that indicate how the energy changes as three reactions occur. Energy Changes for Three Reactions 800 600 Dashboard 400 200 DATE 0 ANALYZING DATA Interpret Energy Diagrams CLASS Direction of reaction 000 000 Calendar DATE .5GE 14 A D Copyright © Savvas Learning Company LLC. All Rights Reserved. Savvas is not responsible for any modifications made by end users to the content posted in its…